Electrolysis Of Copper Sulphate Equation



(10 points) Reactant Balanced Equation Iron (III) and copper (II) sulfate solution 2Fe + 3CuSO4 ----> Fe2(SO4)3 + 3Cu Lead (II) nitrate and potassium iodide solutions Pb(NO3)2 + 2KI ----> PbI2 + 2KNO3 Magnesium metal and hydrochloric acid solution Mg + 2HCl ----> MgCl2 + H2 Electrolysis of water 2H2O ----> 2H2 + O2 Burning. Purification of Copper by Electrolysis (extraction from ore above). Revision Checklist: Chemical Changes Magnesium is more reactive than copper so there is a displacement reaction. ELECTROLYSIS OF COPPER(II) SULFATE SOLUTION - Interactive Flash Animation - Flash simulation to understand what's happen at anode, cathode and salt bridge. Pure copper cathodes are arranged between the blister copper anodes and a current of over 200 A passed through the. Let us take as an example the electrolysis of aqueous copper (II) sulphate solution. There are some ways to make copper sulfate, however. This consists of a 500 mL beaker containing the electrolyte solution into which an inverted burette filled up with the same solution is dipped. Why does the colour of copper sulphate solution change when an iron nail is dipped in it? Write two observations. Here's the half equations to the electrolysis of copper(II) nitrate. copper sulfate solution). Electrical4U 108,224 views. This research is very important, as traditional mining involves huge open-cast mines that produce a lot of waste rock. Copper can be purified using electrolysis. The reaction at the negative electrode is the same but the positive electrode becomes smaller and the solution remains blue. Then we supply electricity from an external source. 2g of Copper was deposited at the cathode, calculate the volume of chlorine gas evolved at the anode at STP at the same time. The second part of this investigation covers the products formed during the electrolysis of copper sulfate solution using inert (graphite) electrodes. This example appears as an answer to another question in Quora. (b) During the electrolysis of aqueous copper (II) sulphate using copper electrodes, a current of 0. The thermochemical equation is shown below, Electrolysis of 0. •The equation is: Mg (s) + CuSO4 (aq) → Cu (s) + MgSO4 (aq) •If you place a copper strip in a solution of magnesium sulfate, no reaction occurs. 1 ELECTROLYSIS G10 worksheet for Electrloysis. Electrolysis question: MgSO4, H20 Hi All, I built a water electrolysis chamber. These are called low grade ores and have less than 1% copper but they are still used because copper is so valuable. Unit C2, C2. A good example is the electrolysis of water. Recall: If the electrolysis of copper (II) sulphate is done using carbon electrodes, oxygen is released at the anode and copper is deposited at the cathode. Write the full name of elements in copper sulphate and radicals followed by its symbols and write a balanced equation for electrolysis of water balance the equation. (a) The electrolysis of lead bromide liberates lead and bromine. 1b Refining copper by electrolysis C6. 50 amps of current through a solution of copper (II) sulfate for 50. 1 the electrolysis of concentrated aqueous sodium chloride 2 the electrolysis of dilute sulfuric acid. !Copper is extracted from copper sulfide. The corresponding equation can be presented as follow:. 635 g of copper at the cathode during the electrolysis of copper(II) sulphate solution if you use a current of 0. *(d) Impure copper can be purified using electrolysis. Copper sulphate solution is ionised by the following chemical equation: CuSO 4 → Cu 2. Attach one electrode to the negative terminal of a dc supply, and the other elec-trode to the positive terminal. 4 7 g of C u O was obtained by oxidising 1. PubChem: 8895 Chemical equation: 2CH 3 COOH + Cu —electrolysis→ Cu(CH 3 COO) 2 + H 2 ↑ For preparation of 100. The four amounts of copper sulfate tested were 5g, 10g, 15g,and 20g dissolved in 150mL of water. Solution: (Based on the StoPGoPS approach to problem solving. A simple method of investigating the electrolysis of Basic Copper Chloride (WSDTY) solution is described. power supply, a switch and electrical wires for the external circuit. The reaction that forms the oxygen (2H 2 O -> 4H + + O 2 + 4e - ), as Borek stated, means that the concentration of hydrogen ions increases and, thus, increases the pH. Why does the colour of copper sulphate solution change when an iron nail is dipped in it? Ans. (b) During the electrolysis of aqueous copper (II) sulphate using copper electrodes, a current of 0. Place two graphite rods into the copper sulfate solution. e sulphuric acid is also produced. The equation for the €€€€ The student knew that copper sulphate, €€€€€€€€€ The electrolysis of sodium chloride solution is an. Faraday's Laws of Electrolysis Tutorial Key Concepts. (i) *describe the electrolysis of aqueous copper(II) sulfate with copper electrodes as a means of purifying copper (j) *describe the electroplating of metals, e. Example: Electrolysis of copper II sulphate solution. Electricity is passed through aqueous sodium chloride solution (brine). We take two copper electrodes and place them into a solution of blue copper sulfate (CuSO 4) and then turn the current on. Once the anode and cathode have been determined, the cathode can be replaced by a conducting item such as a key. 30 min using a current of 2. The metallic copper produced will be weighed. In another beaker a plate of copper is dipped in a solution of copper (II) sulfate in another container. If equation (1) is correct, the moles of copper should equal the moles of iron. Learn faster with spaced repetition. The overall balanced equation Predict the product formed at the positive electrode during the electrolysis of concentrated sodium sulfate. (c) Copper sulphate on treatment with potassium iodide precipitates cuprous iodide (Cu2 I2), liberates iodine gas and also forms potassium sulphate. During the electrolysis of […]. In this classic experiment, from the Royal Society of Chemistry, students electrolyse copper sulphate solution using carbon electrodes. Refining Copper and Electroplating (DEMO) Relate the products of electrolysis to the electrolyte and electrodes used using carbon electrodes and using copper electrodes (as used in the refining of copper) Introduction Active electrodes are electrodes which participate in the reaction. I do have an idea of what's going on, but I'd rather this was just explained. negative electrode copper sulfate solution State the name given to a positive electrode. One example of reactive electrodes changing the ionic discharge will be the electrolysis of Copper (II) sulphate using copper electrodes. Electrolysis of copper (II) sulphate solution using copper electrodes Apparatus and chemicals: Copper foils as electrodes, copper(II) sulphate solution, Dry cells or car battery. Electrolysis of silver sulphate solution, Ag2SO4 using silver electrode as anode and carbon electrode as cathode. 10) Photosynthesis is considered an endothermic reaction because energy in the form of sunlight is absorbed by the green plants. This experiment enables students to carry out the electrolysis of copper (II) sulfate solution and to link their findings with the industrial electrolytic refining of copper. This salt exists as a series of compounds that differ in their degree of hydration. Here's the half equations to the electrolysis of copper(II) nitrate. A dilute aqueous solution of copper sulfate and sulfuric acid is used as the electrolyte. A student conducts an investigation to find out what is produced during the electrolysis of sodium sulfate. Therefore, the blue colour of copper sulphate solution fades and green colour appears. Electrolysis of water 5. Silver metal. Quantitative electrolysis of aqueous copper(III) sulfate Questions for students 1 Calculate the number of moles of copper removed from the anode (weight lost (g)/ A r [Cu]). (i) *describe the electrolysis of aqueous copper(II) sulfate with copper electrodes as a means of purifying copper (j) *describe the electroplating of metals, e. The diagram below shows a cell that can be used for this process. During the electrolysis of Copper (ll) chloride solution, 3. The net effect is the transfer of copper from electrode X to electrode Y. A colourless gas is produced at the negative electrode. Electrolysis of Copper Sulfate Whenever copper sulfate or CuSO 4 is added to water, it gets dissolved in the water. The copper electrodes are "active" meaning they take a part in the electrolysis. The two electrodes are connected via wire. copper|copper sulphate half cell Eº = +0,34 V E cell = the difference between the two values = 1,10 V Direction of electron flow will be from the better reducing agent i. Ions move through the membrane to maintain electrical neutrality in the cell. 1 M sulfuric acid solution is carried out using copper electrodes and a simple experimental setup. Electrolysis of copper sulfate in soil February 2, 2010. Electrolysis: Splitting Water Student Version • Writing down balanced chemical reactions is useful for figuring out relative quantities of products formed. Describe how the student could carry out an. 30 Explain the formation of the products in the electrolysis of copper sulfate solution, using copper electrodes, and how this electrolysis can be used to purify copper; Edexcel Combined. The student weighed the copper sulfate crystals when they were wet. Calculate the concentration of copper sulphate in the solution to begin with. The net effect is the transfer of copper from electrode X to electrode Y. Copper ions and sulfate ions. Tick (€ ) the one statement that explains why the mass of copper sulfate crystals was less than expected. Two graphite electrodes were connected to a D. The reaction equation for chalcopyrite is as follows: CuFeS 2 + 4Fe +3 ➝Cu + + + 5Fe + + 2S° the resulting nonporous sulfur product layer surrounding each particle of the copper concentrate acts to block the reaction which, as a result, severely limits the amount of copper which can be extracted from the concentrate. Copper ions and sulfate ions. It is used for measuring electrode potential and is the most commonly used reference electrode for testing cathodic protection corrosion control systems. The anode (positive electrode) is made from impure copper and. pdf), Text File (. This involves setting up an electrolysis to investigate the effect of changing the current on the mass of the copper electrodes used in the electrolysis of copper sulfate solution. Two iron nails that were cleaned by rubbing with sand paper were immersed into test tube B and left undisturbed for 20 min. The positive copper ions move towards the negative electrode where they gain electrons, forming solid copper. The cathode is a thin piece of pure copper. 00 A to plate out all of the silver from 0. An aqueous solution of a compound contains (a) anions and cations of the compound. Which statement is correct about the electrolysis of Copper (II) Sulphate solution using graphite electrodes? A. In chemistry, electrolysis is a method that uses a DC to drive a non-spontaneous chemical reaction. Copper sulfate is an ionic compound composed of copper, sulfur, and oxygen. At the cathode, copper(II) ions will be deposited, hence a brown solid is formed at the cathode. Hydrogen and oxygen can be obtained by electrolysis of acidified water. A student conducts an investigation to find out what is produced during the electrolysis of sodium sulfate. The ionic compound must be molten or dissolved in water to allow the ions to be mobile, since it is the movement of ions that is needed for electrolysis to occur. The sodium ions and sulfate ion are the spectator ions in this reaction. Completely fill two small test tubes with copper sulfate solution and position a test tube over each electrode. which indicates that the zinc reacts with the copper sulphate solution to produce copper and zinc sulphate solution. € (1) (Total 6 marks. To understand the concept of electrolysis let us take an example of a common electrolyte like copper sulfate (CuSO 4). At the inert anode, oxygen from the water is oxidized to oxygen gas. At the Cathode: 4OH-- 4e-→ O 2 + 2H 2 O Oxygen from OH-ions is formed. Use Simultaneous Equations technique to balance off the electrons and you will end up with the Overall Reaction Equation for electrolysis. Together, they cited 16 references. 5M hydrochloric acid rather than the 100mL of 0. Sodium can be prepared by electrolysis only were as iron fro blast furnace give your answer (in terms of reactivity) 15. You can make other things out of it. Electrorefining of Copper 1. the electrode reactions are, at the anode: M → Mn+ + ne-and at the cathode: Mn+ + ne-→ M. 4 7 g of C u O was obtained by oxidising 1. Causes hydroxylamine to ignite. 5 Amp Current Is Used For 30 Minutes. A constant current of 2 mA was passed for 19. This article has also been viewed 153,868 times. To do this we need the solution of copper sulfate CuSO 4, which contains dissolved copper. The copper(II) ions are removed again from the organic solvent by reaction with fresh sulfuric acid, producing a much more concentrated copper(II) sulfate solution than before. Electrolysis can also be used to purify metals. These were then placed into a beaker of blue copper sulfate solution (2M). Electrolysis of a copper(II) nitrate solution produces oxygen at the anode and copper at the cathode. The electrolysis is similar to that of copper (II) sulfate solution with inert electrodes. calcium most reactive aluminium zinc iron copper gold least reactive. 0 M Copper(i) Sulfate Solution Given That A 2. The products formed in the electrolysis of aqueous CuSO 4 are Cu(s) and O 2 (g). Hydrogen and oxygen can be obtained by electrolysis of acidified water. Gcse Chemistry – Electrolysis Coursework. Calculate masses deposited in electrolysis (see also chapter E3). Explain how Equation 2a turns into Equation 2b. The net effect is the transfer of copper from electrode X to electrode Y. The element that is reduced gains electrons, while element that is oxidized loses electrons. It is found in the Earth’s crust as an ore which contains copper sulfide. COPPER SULFATE PENTAHYDRATE can be dehydrated by heating. Electrolysis of copper sulphate solution Electrolysis is the chemical decomposition of an ionic compound by passing an electric current through it. It was found that after electrolysis the absorbance of the solution was reduced to 50 % of its original value. (A purity of 99. mass of electrode before electrolysis / g mass of electrode after electrolysis / g change in mass mass of impure copper anode 40. Copper sulphate solution (250 ml) was electrolysed using a platinum anode and a copper cathode. 022 x 10 23 words. Oxidation half-equation Zn (s) → Zn2+ (aq) + 2e-. In another beaker a plate of copper is dipped in a solution of copper (II) sulfate in another container. Diagram 2 (a) Write the formula of all the ions present in the copper(II) sulphate solution. bubbles of oxygen are given off at the anode As the copper ions are discharged as copper atoms at the cathode, the blue colour of the solution gradually fades and an oxidation reaction occurs which is the 4e- (electron loss). These are dipped into an electrolyte of copper(II) sulphate solution. iv: Deduce the half-equations for the reactions occurring at the positive electrode (anode) and. It was found that after electrolysis the absorbance of the solution was reduced to 50 % of its original value. These were then placed into a beaker of blue copper sulfate solution (2M). The solution becomes sulphuric acid because copper(II) ions and hydroxide ions are consumed in the electrolysis. equation for the reaction at the positive electrode in copper sulphate. 4 > were determined. The single replacement reaction of Magnesium and Copper Sulfate produce:Mg + CuSO4 → MgSO4 + CuTheoretically, if Magnesium is placed in Copper Sulfate solution, a single replacement reaction occurs. If we use coal of platinum electrodes, the reactions are as follows:. (A purity of 99. Practice Redox Problem: balance the following redox reaction in acidic solution: S(s) + NO 3-(aq) --> SO 2 (g) + NO(g). The charge on the silver ion was 1+. Some solutions release noxious or explosive gases on electrolysis, some are hazardous in themselves. Electrolysis of a copper(II) nitrate solution produces oxygen at the anode and copper at the cathode. 3 Galvanic and electrolytic cells (ESCR3) Electrochemical reactions (ESCR4) In Grade 11, you carried out an experiment to see what happens when zinc granules are added to a solution of copper(II) sulfate. > You have a mixture of "Cu"^"2+", "SO"_4^"2-", and "H"_2"O". (6) Sodium sulfate solution contains sodium ions, Na+, sulfate ions, SO4 2–, hydrogen ions, H+, and hydroxide ions, OH–. Task 3: Replicate activity 3 and manipulating the distance of copper metal with iron nail. The pure copper cathode increases greatly in size, while the anode dwindles away. Overall equation for the electrolysis of copper (II) sulfate solution:. Pick the correct half equations for the electrolysis of copper sulfate using copper electrodes. Thus, Copper Sulphate reacts to form iron (ii) Sulphate, the blue colour of copper sulphate Solution fades. 3 3 5 g copper was precipitated by 0. Electrolysis of copper sulfate in soil February 2, 2010. Faraday's Laws of Electrolysis Tutorial Key Concepts. In addition, copper sulfate was reported to be used as a processing aid in alcoholic beverages. The electrolysis of copper(II) sulphate solution using a copper anode. • Write the half equation. 9 8 6 g of copper by nitric acid. At the cathode: Copper(II) ions are reduced to form copper metal, which is deposited on the object. Two copper strips are dipped in an aqueous solution ofcopper sulphate (CuSO 4). Both forms are incompatible with finely powdered metals. Designed to accompany a short practical session with students predicting what they think will happen. Electrolysis. Cu + H 2 SO 4 → CuSO 4 + H 2. A copper deposit. The copper sulphate is ionised in aqueous solution. Metal ions less reactive than. Bubbles of gas were seen to. Electrolysing Copper(II) Sulfate Solution In this classic experiment, from the Royal Society of Chemistry, students electrolyse copper sulphate solution using carbon electrodes. Then we supply electricity from an external source. Electrolysis of Copper(II) Sulfate Solution: Ions present in the electrolyte are H + and OH-from water and Cu +2 and SO 4-from copper(ii) sulfate. Include cell diagram, observations, anode and cathode reactions and state the uses. (A purity of 99. The plants absorb copper compounds through their roots. asked by Marisol on March 28, 2007; can u help me write a word equation for the electrolysis of water , and indicate physical states and. Electrolysis is the process by which an electric current is passed through a substance to affect a chemical change. Of all the stuff to try to synthesize! Just buy the copper sulfate, it is available at hardware stores for reasonable prices in excellent purity. Calculate the concentration of copper sulphate in the solution to begin with. Gcse Chemistry – Electrolysis Coursework. Decomposition of sodium chloride:On passing electricity through molten sodium chloride, it decomposes into sodium and chlorine. € € Statement Tick ( ) € Some copper sulfate may have been lost during the experiment. Magnesium metal ribbon and hydrochloric acid solution Mg + 2 HCl = MgCl2 + H2 4. using active electrodes) results in transfer of copper metal from the anode to the cathode during electrolysis. Iron + Copper Sulphate –> Iron(ii) Sulphate + Copper. BASIC ELECTROLYSIS CALCULATIONS - chemguide Answer: During electrolysis of aqueous copper sulphate using copper electrodes, the two anions OH –. It was found that after electrolysis the absorbance of the solution was reduced to 50 % of its original value. The electrolysis of many salts (e. Introduction: Prior to understanding the Faraday's laws of electrolysis, we have to revise the procedure of electrolysis of a metal sulphate. So the negative electrode gets this thin copper layer on it. In the two experiments listed below, the first reactive substance is water and the second one is a copper sulfate solution. Prepare a solution of copper sulphate, put in it the electrodes and turn on the power supply. Platinum anodes were not inert at certain combinations of temperature and current density, and platinum acted as a low overvoltage impurity. This investigation will examine one of the factors that affect the amount off copper deposited during the electrolysis of copper (II) sulphate solution. Quantitative electrolysis of aqueous copper(III) sulfate Questions for students 1 Calculate the number of moles of copper removed from the anode (weight lost (g)/ A r [Cu]). Then, when you apply electricity and a copper ion is touching your nickel cathode, two electrons flow into it reducing it from a Cu ++ ion to a Cu 0 metal atom. 4 7 g of C u O was obtained by oxidising 1. Faraday’s Laws of Electrolysis. When copper electrodes are used in the electrolysis of copper sulfate solution, the mass loss of copper from the positive anode electrode should equal the mass of copper gained and deposited on the negative cathode electrode. using active electrodes) results in transfer of copper metal from the anode to the cathode during electrolysis. Together, they cited 16 references. When a nickel strip {Ni (s)} is placed in an aqueous solution of copper(II) sulfate {Cu 2+, SO 4 2-}, an immediate reaction occurs. 2) takes place in a constant volume container using 1 kmol Zn (45 kg Zn) then 214,852 kJ of heat must be transferred from the container to. At the cathode a shiny orange layer is formed. The following reaction takes place when zinc is placed in a copper sulfate solution: Zn + Cu 2+ → Zn 2+ + Cu In the electrolysis of copper sulfate solution using copper electrodes, which one of the following reactions takes place at the cathode?. The electrolysis of an aqueous solution of copper sulphate using copper electrodes (i. The reaction between the two elements in an electrolytic cell is a reduction-oxidation -- or redox -- reaction. Bromthymol blue (BTB) has been added to the other solution. Identify any elements and compounds in the. Each group of students will require: Beaker (250 cm3). One example of reactive electrodes changing the ionic discharge will be the electrolysis of Copper (II) sulphate using copper electrodes. This example appears as an answer to another question in Quora. (b) What volume of oxygen gas (measured at STP) is produced by the oxidation of water at the anode in the electrolysis of copper(II) sulfate in part (a)? 2. This is a non-spontaneous reaction. 30 min using a current of 2. Given cu=64, 1F=96500C. In this case, the aluminum is obtained from an ore called bauxite. (c) Calcium nitrate reacts with sodium sulphate to form calcium sulphate (same is required in two places). electrolysis o f water Water is a weak electrolyte because it conducts very little amount of electric current. 4 7 g of C u O was obtained by oxidising 1. We are going to look carefully at what happens with two liquids, water and copper sulphate, but first the general ideas. It was found that after electrolysis the absorbance of the solution was reduced to 50 % of its original value. The formation of the products of electrolyzing aqueous copper chloride is fully explained with the appropriate electrode equations. If we use carbon electrodes, they will be inert electrodes and will not affect the electrolysis. 5! Introduction: There are many different factors that can affect the mass of copper deposit on the graphite electrode after electrolysis reaction of copper sulphate such as the increase in voltage, the concentration of ions in electrolyte, surface area of. How many minutes does it take to plate 0. 6 Explaining the electrolysis of aqueous copper sulfate using graphite and copper electrodes. Tick (€ ) the one statement that explains why the mass of copper sulfate crystals was less than expected. Electrolysis uses an electrical current to move ions in an electrolyte solution between two electrodes. The electrolyte is copper sulfate. Some copper ores may contain only small amounts of copper. The reaction at the negative electrode is the same but the positive electrode becomes smaller and the solution remains blue. I chose the Copper Sulfate Electrolyte, a Copper Anode, a Steel Cathode and a Battery as the components in the illustration of a circuit on Electroplating. Copper sulphate solution (250 ml) was electrolysed using a platinum anode and a copper cathode. Introduction: Prior to understanding the Faraday's laws of electrolysis, we have to revise the procedure of electrolysis of a metal sulphate. In this exercise, the electrolysis of a 0. This consists of a 500 mL beaker containing the electrolyte solution into which an inverted burette filled up with the same solution is dipped. 6 Explaining the electrolysis of aqueous copper sulfate using graphite and copper electrodes. Use the beaker to collect about 50 mL of water. A constant current of 2 mA was passed for 19. Electrolysis is a chemical process where a substance in its molten state or in an aqueous solution decomposed by electric current. c electrical current is passed through the solution electrolysis takes place. [Show full abstract] electrolysis from a linear graphite cathode in a 2D film of zinc sulfate solution toward a thick zinc metal anode. 30 Explain the formation of the products in the electrolysis of copper sulfate solution, using copper electrodes, and how this electrolysis can be used to purify copper; Edexcel Combined. This particular experiment involves the electrolysis of copper (II) sulphate using a pair of copper electrodes. • use 100mL of 0. Then we supply electricity from an external source. Procedure. This occurs after oxidizing the copper in sulfuric acid with copper sulfate. Pour some copper sulfate solution into a beaker. efficiency in the electrolysis of pure zinc sulfate solu­ tions (65 gpl Zn++ - 200 gpl H2. Which one of the following best describes what happens at the cathode?. The current is turned on for a period of time. Electrolysis of potassium nitrate solution, KNO 3 using carbon electrodes. This investigation will examine one of the factors that affect the amount off copper deposited during the electrolysis of copper (II) sulphate solution. Both anode and cathode are suspended in a large tank of the copper sulfate solution. COPPER SULFATE PENTAHYDRATE can be dehydrated by heating. So the negative electrode gets this thin copper layer on it. Hydrogen and oxygen can be obtained by electrolysis of acidified water. Learn faster with spaced repetition. equation for the reaction at the positive electrode in copper sulphate. > You have a mixture of "Cu"^"2+", "SO"_4^"2-", and "H"_2"O". These electrodes behave as terminal to hold the electrons. These were then placed into a beaker of blue copper sulfate solution (2M). KOH(aq) + H 2 SO < (aq) KHSO < (aq) + H 2 O(l) Suggest how you could make a solution of potassium hydrogen sulfate without using an indicator. It was found that after electrolysis the absorbance of the solution was reduced to 50 % of its original value. Electrolysis has three component a Cathode, an Anode, and the electrolyte solution. Which one of the following best describes what happens at the cathode?. Nickel is a close metal to iron and so is lower down in the reactivity series. Of all the stuff to try to synthesize! Just buy the copper sulfate, it is available at hardware stores for reasonable prices in excellent purity. € In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. - Electrolysis Investigation To monitor the quantity of copper (Cu) metal deposited during the electrolysis of copper sulphate solution. Pick the correct half equations for the electrolysis of copper sulfate using copper electrodes. Together, they cited 17 references. Copper(II) sulfate. Calculate the concentration of copper sulphate in the solution to begin with. Electrolysis of Copper (II) Sulphate? When Copper (II) Sulphate is electrolysed with carbon electrodes a colourless gas is given off at the anode and the solution goes from blue to colourless. The copper sulphate is ionised in the aqueous solution. 31 Investigate the electrolysis of copper sulfate solution with inert electrodes and copper electrodes; Topic 3 - Chemical changes. The electrolysis of copper(II) sulfate solution. The pentahydrate (x = 5) is the most common form. Lesson organisation. A constant current of 2 mA was passed for 19. Hydrogen ion from the acid solution will receive the electrons. Why does the colour of copper sulphate solution change when an iron nail is dipped in it? Ans. 4 7 g of C u O was obtained by oxidising 1. A student carried out the electrolysis of copper sulfate using inert electrodes. Instead of using inert electrodes, chemists tried placing pure copper electrodes in copper sulphate solution. Made of the most DURABLE PLASTICS , the Half Cells will withstand severe abuse without damage. 4 the purification of copper using aqueous copper(II) sulfate. Even after electrolysis, the sulfate anion is not removed. 1 M sulfuric acid solution is carried out using copper electrodes and a simple experimental setup. This consists of 1 mark Questions, 3 Mark Numericals Questions, 5 Marks Numerical Questions and previous year questions from Chemical Reactions and Equations Chapter. The electrolysis of many salts (e. The fiber industry uses it for creating synthetic fibers. One method of purifying copper is by electrolysis. Aim: To extract the copper from copper sulphate using the process of electrolysis. There are small concentrations of hydrogen ions H + and hydroxide ions (OH -) from the self-ionisation of water itself, but these can be ignored in this experiment. 2a and 2b show the kinetic results of copper electrodeposition (i. Is copper sulphate a reactant or a product in the following equation copper sulphate plus sodium hydroxide equals copper hydroxide plus sodium sulphate? Copper sulfate is a reactant in the equation as stated, because it is present before the reaction has occurred and no longer present afterward. Hydrogen and oxygen can be obtained by electrolysis of acidified water. Explain how these products are formed from the ions in the electrolysis process, indicating how you would identify the products. the electrode connected to the negative terminal of the battery. The plants are burned to produce copper oxide. e sulphuric acid is also produced. Chemical Reactions and Equations Chapter wise important question for Class 10 Science PDF will help you in scoring more marks. equation for the reaction at the positive electrode in copper sulphate. (a) Calculate the mass of copper metal produced at the cathode during the passage of 2. This time you can’t start by working out the number of coulombs, because you don’t know the time. Copper ions and sulfate ions. € (1) (Total 6 marks. Copper sulphate solution (250 ml) was electrolysed using a platinum anode and a copper cathode. We measure the distance between adjacent trees, calculate. The removal was larger at higher pH o. Electrolysis of concentrated potassium chloride solution, KCl using carbon electrodes. A mixture of magnesium sulfate and zinc nitrate with graphite electrodes. Copper(II) sulfate, also known as cupric sulfate or simply copper sulphate, is the chemical compound with the chemical formula CuSO 4. A better description of this is that. The second part of this investigation covers the products formed during the electrolysis of copper sulfate solution using inert (graphite) electrodes. Something must be oxidized, and something must be reduced, so you consult a table of standard reduction potentials like the one below to find suitable candidates, The only candidate for reduction in the table is "Cu"^"2+""(aq)" + 2"e"^"-" → "Cu(s)"; "+0. Using equations for the reactions at the electrodes, explain why the volume of hydrogen obtained is twice that of oxygen. Electricity is passed through aqueous sodium chloride solution (brine). (d) Crystals of sulphur are obtained when a solution of sulphur in carbon disulphide is allowed to evaporate. The Electrolysis of Copper Sulphate Aim Analyse and evaluate the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when certain variables were changed. This involves setting up an electrolysis to investigate the effect of changing the current on the mass of the copper electrodes used in the electrolysis of copper sulfate solution. (c) Calcium nitrate reacts with sodium sulphate to form calcium sulphate (same is required in two places). In electrolysis ionic compounds are broken down. (in this equation the iron oxide is being reducedand the carbon monoxide is causing the reduction) Metals that are less reactive than carbon can be extracted from their oxides by reduction with carbon 4. 10) Photosynthesis is considered an endothermic reaction because energy in the form of sunlight is absorbed by the green plants. When copper electrodes are used the action at the cathode is exactly the same as with platinum or carbon electrodes. Electrolysis of water 5. Add one spoonful of copper sulfate powder to the water. (2) (Total 5 marks) 26. How long would it take to deposit 0. The positive copper ions move towards the negative electrode where they gain electrons, forming solid copper. These electrodes behave as terminal to hold the electrons. Extraction of Metals. The overall reaction is: 2Cu+2(aq) + 2H2O = 4H+(aq) + O2(g) +2Cu(s). These plates of metal are called the electrodes of the cell. The electrolysis of an aqueous solution of copper sulphate using copper electrodes (i. power supply, one to the anode (+ve terminal) and the other to the cathode (-ve terminal). copper sulfate solution). Platinum anodes were not inert at certain combinations of temperature and current density, and platinum acted as a low overvoltage impurity. • Write the half equation. At the cathode, copper(II) ions will be deposited, hence a brown solid is formed at the cathode. The electrolyte does not change colour. Colourless gas bubbles are released. Electrolysis is also used in electroplating. The power supply was switched on and a potential difference of 12 volts was applied. Electrolysis of copper sulfate and its use to refine blister copper by electrolytic refining. This reaction causes copper metal (brown) to be deposited on the negative electrode while bubbles of chlorine gas are produced at the positive electrode. Designed to accompany a short practical session with students predicting what they think will happen. A DC voltage is applied to both the electrodes. There are small concentrations of hydrogen ions H + and hydroxide ions (OH –) from the self-ionisation of water itself, but these can be ignored in this experiment. 0 g of copper at the cathode of an electrolysis cell containing CuSO 4(aq) using a current of 20 000 mA. COPPER SULFATE PENTAHYDRATE can be dehydrated by heating. Here's a simplified diagram for the electrolysis of molten Sodium chloride. Copper sulphate solution (250 ml) was electrolysed using a platinum anode and a copper cathode. 2 H(+) + 2 e(-) ==> H2- At the anode the concentration of Hydroxyl Ions, HO(-),is too low to maintain a reaction and the Sulphate Ions, SO4(2 -) are not oxidized but remain on in. Chloride ions, potassium ions, copper(II) ions, zinc ions, zinc atom and copper atom. Explain how these products are formed from the ions in the electrolysis process, indicating how you would identify the products. For instance the electrolysis of copper sulphate is OK with copper electrodes but the sulphuric acid requires platinum electrodes or they will be eaten away. copper|copper sulphate half cell Eº = +0,34 V E cell = the difference between the two values = 1,10 V Direction of electron flow will be from the better reducing agent i. The electrolysis of copper(II) sulphate solution using copper electrodes A copper atom breaks away from the electrode forming a copper(II) ion, leaving its electrons behind on the electrode. 9 8 6 g of copper by nitric acid. A direct electric current is passed through the solution. 50 amps of current through a solution of copper (II) sulfate for 50. Calculate the moles of copper metal that can be produced by the electrolysis of molten copper sulfate using 500 C of electricity. Quantitative analysis when using copper electrodes will be expected. To create this article, 48 people, some anonymous, worked to edit and improve it over time. removal) at a rate of flow of 0. Which processes produce oxygen at one of the electrodes?. The impure copper from a smelter is cast into a block to form the positive anode. The word "electrolysis" was introduced by Michael Faraday in the 19th century. Similarly, fine copper shaken in ammoniacal air is said to produce a rapid oxidation of both the ammonia and copper (into "nitrite of copper'). Given the stable and readily available nature of copper sulfate, it makes an inexpensive school laboratory material and eliminates the chlorine gas risk associated with. An electrolytic cell for refining copper contains very pure copper at the cathode, impure copper at the anode, and copper sulfate as the electrolyte. [Show full abstract] electrolysis from a linear graphite cathode in a 2D film of zinc sulfate solution toward a thick zinc metal anode. 5M hydrochlric acid used in Part 1 What's Going On Figure 7 Figure 7 is a diagram of the process you have used to plate zinc onto copper. Those electrons can then be pumped away by the power source around the circuit to the cathode. Therefore, the blue colour of copper sulphate solution fades and green colour appears. There are small concentrations of hydrogen ions H + and hydroxide ions (OH –) from the self-ionisation of water itself, but these can be ignored in this experiment. No, copper sulfate can't form on electrical wires. Write a balanced equation for each reaction observed in this lab. The lattice can accommodate ions of a different metal. Electrolysis of Copper (II) sulphate solution Copper (II) sulphate solution can be electrolysed using inert platinum electrodes. Iron displaces copper from copper sulphate solution and forms pale green coloured solution of FeS04 and reddish brown copper metal gets deposited. Which one of the following best describes what happens at the cathode?. The Journal of Physical Chemistry 1916, 20 (4) , 296-322. Another alternative for students to understanding an abstract concept in chemistry. > You have a mixture of "Cu"^"2+", "SO"_4^"2-", and "H"_2"O". 5 Do not write outside the box (05) G/Jun17/CH2FP Turn over 2 This question is about sulfuric acid, copper sulfate and ethene. Not sure it would be thermally stable to it's melting point. It was found that after electrolysis the absorbance of the solution was reduced to 50 % of its original value. molten copper(II) chloride, CuCl2 2) At the cathode: • This negatively charged electrode attracts the Cu2+ ions • The cathode gives 2 electrons to each Cu2+ ion •The Cu2+ ions become Cu atoms and are deposited on the cathode. How do I make this a proper reaction equation? Thanks. And the positive electrode just kinda starts to turn into copper ions and dissappear into the solution. 3 3 5 g copper was precipitated by 0. iii: State why copper electrodes cannot be used in the electrolysis of water. Cu = Cu+2 + 2e- what type of material are the electrodes in the electrolysis of acidified water. Iron + lithium sulphate. Electrolysis of copper chloride is a way of splitting up decomposition of the compound copper chloride using electrical energy. 999 percent is not unusual. The formation of the products of electrolyzing aqueous copper chloride is fully explained with the appropriate electrode equations. using active electrodes) results in transfer of copper metal from the anode to the cathode during electrolysis. 5! Introduction: There are many different factors that can affect the mass of copper deposit on the graphite electrode after electrolysis reaction of copper sulphate such as the increase in voltage, the concentration of ions in electrolyte, surface area of. This research is very important, as traditional mining involves huge open-cast mines that produce a lot of waste rock. Which statement is correct about the electrolysis of Copper (II) Sulphate solution using graphite electrodes? A. At the anode: Cu. The two electrodes are connected via wire. Investigate what happens when aqueous solutions are electrolysed using inert electrodes. At the inert anode, oxygen from the water is oxidized to oxygen gas. If equation (1) is correct, the moles of copper should equal the moles of iron. Gains water readily. 00g of copper(II) sulfate pentahydrate. Prepare a solution of copper sulphate, put in it the electrodes and turn on the power supply. Electrolysis if Copper Sulfate. How many minutes does it take to plate 0. Copper sulfate sodium hydroxide - Answers. Please note that in the half-equations, the equal '=' sign should be an arrow '-->'. Electrolysis of water: Electrolysis of water is the decomposition of water into hydrogen and oxygen due to the passage of electric current through it. 44V of water to from hydrogen : -0. When copper electrodes are used in the electrolysis of copper sulfate solution, the mass loss of copper from the positive anode electrode should equal the mass of copper gained and deposited on. The copper sulphate is ionised in aqueous solution. And the positive electrode just kinda starts to turn into copper ions and dissappear into the solution. Copper Sulphate Electrolysis (Cathode) Word Equation: Copper (II) ion + electrons → Copper metal : Ionic Half Equation: Cu 2+ (aq) + 2e-→ Cu (s) Description. Copper gluconate and copper sulfate were reported to be used as nutrients in milk products, processed fruit juices and drinks, soft candy, snack foods, beverages, chewing gum, and baby and infant formula. A direct electric current is passed through the solution. Can you write the half equations for each of the electrode?. What are the products of the electrolysis of aqueous copper ch. The blue colour of the solution fades gradually as more. Hypothesis: I think that one if the carbon rod will change. Two iron nails that were cleaned by rubbing with sand paper were immersed into test tube B and left undisturbed for 20 min. Not sure it would be thermally stable to it's melting point. (a) The electrolysis of lead bromide liberates lead and bromine. The power supply was switched on and a potential difference of 12 volts was applied. 59C write ionic half-equations representing the reactions at the electrodes during electrolysis and understand why these reactions are classified The electrolysis of dilute Copper Sulphate (CuSO 4) Cations. If you are using impure copper for an anode the reaction will be. The electrolysis of an aqueous solution of copper sulphate using copper electrodes (i. Three electrolysis cells are connected in series. When copper electrodes are used in the electrolysis of copper sulfate solution, the mass loss of copper from the positive anode electrode should equal the mass of copper gained and deposited on the negative cathode electrode. One example of reactive electrodes changing the ionic discharge will be the electrolysis of Copper (II) sulphate using copper electrodes. The same holds for the copper sulfate and sulphuric acid. The Cu 2 + from the anode moves through a sulfuric acid-copper(II) sulfate solution into the cathode where it becomes solid copper. The method used to extract a metal from its ore is linked to the reactivity of the metal. The hydrated salt is vigorously reduced by hydroxylamine [Mellor 8:292(1946-1947)]. Electrolysis of copper sulphate solution Electrolysis is the chemical decomposition of an ionic compound by passing an electric current through it. Chemistry Form 4 experiment chapter 6 (6. A constant current of 2 mA was passed for 19. Carbon electrodes (black) submerged in a solution of copper chloride and connected to a power supply (not shown). Chemical Reaction Observations Reaction Type Iron and copper (II) sulfate solution The iron turned a brownish red color Single displacement Lead (II) nitrate and potassium iodide solutions It went toward the bottom of the test tube, and the solution appeared as a thick opaque yellow Double displacement Magnesium metal and hydrochloric acid solution Magnesium had bubbles forming around it, as. Aim: To extract the copper from copper sulphate using the process of electrolysis. • The order of reactivity of the metals can be confirmed (most reactive first): Mg, Zn, Fe and then Cu. 3 4 6 g of zinc from C u S O 4 solution. The impure copper is made the anode (+) and a thin piece of pure copper is made the cathode (−). This experiment enables students to carry out the electrolysis of copper (II) sulfate solution and to link their findings with the industrial electrolytic refining of copper. Write a balanced equation for each reaction observed in this lab. The net effect is the transfer of copper from electrode X to electrode Y. (They provided the reactants, my answer is the products) Iron(s) + copper sulfate(aq) → iron. Study Electrolysis Experperiment 1 (Sodium Sulfate Solution) flashcards from Cathal O'Leary's class online, or in Brainscape's iPhone or Android app. The copper. Older names for this compound include blue vitriol, bluestone, vitriol of copper, and Roman vitriol. In this part of the electrolysis of aqueous solutions lab, you see the electrolysis of two aqueous sodium sulfate solutions. (6) Sodium sulfate solution contains sodium ions, Na+, sulfate ions, SO4 2–, hydrogen ions, H+, and hydroxide ions, OH–. 8 g increase Explain these results. purification of ores such as copper sulfide ore. An example of active electrodes is in the electrolysis of copper sulfate solution with copper electrodes. A student conducts an investigation to find out what is produced during the electrolysis of sodium sulfate. The electrolysis of an aqueous solution of copper sulphate using copper electrodes (i. 00 A to plate out all of the silver from 0. -) The positively charged copper ions migrate to the cathode, where. If you seperated a magnesium sulfate solution through electrolysis with a copper anode you would in return get a copper sulfate solution and a magnesium hydroxide precipitate MgSO4(aq) + 2 H2O + Cu(s) → H2(g) + Mg(OH)2(s) + CuSO4(aq) But do. + + (cation) and SO. The ionic equation for the reduction process:Cu2+ (aq) + 2e - --> Cu (s) Reduction of copper ion produces copper atom. (10 points) Reactant Balanced Equation Iron (III) and copper (II) sulfate solution 2Fe + 3CuSO4 ----> Fe2(SO4)3 + 3Cu Lead (II) nitrate and potassium iodide solutions Pb(NO3)2 + 2KI ----> PbI2 + 2KNO3 Magnesium metal and hydrochloric acid solution Mg + 2HCl ----> MgCl2 + H2 Electrolysis of water 2H2O ----> 2H2 + O2 Burning. A glowing splint thrust into the copper gas burst into flame, while a glowing splint approaching the zinc gas caused a loud "pop. The third solution is made from dissolved copper (II) sulfate (CuSO 4). Copper II ions are deposited as copper on the cathode for the electrode equation see under the purification of copper below. (a) A student was given two different types of electrodes (carbon and copper electrodes) to carry out electrolysis of copper(II) sulfate solution. The equation for the €€€€ The student knew that copper sulphate, €€€€€€€€€ The electrolysis of sodium chloride solution is an. iii) Nature of the Electrode. The reaction that forms the oxygen (2H 2 O -> 4H + + O 2 + 4e - ), as Borek stated, means that the concentration of hydrogen ions increases and, thus, increases the pH. The anodes for this process were traditionally lead-based alloys, but newer methods use titanium or stainless steel. It is equivalent to 9. Platinum anodes were not inert at certain combinations of temperature and current density, and platinum acted as a low overvoltage impurity. The electrode reactions and products elcetrolysis the electrolysis of copper chloride solution are illustrated by the theory diagram above. Something must be oxidized, and something must be reduced, so you consult a table of standard reduction potentials like the one below to find suitable candidates, The only candidate for reduction in the table is "Cu"^"2+""(aq)" + 2"e"^"-" → "Cu(s)"; "+0. A grey solid is formed. 3 3 5 g copper was precipitated by 0. Iron + Copper Sulphate –> Iron(ii) Sulphate + Copper. Introduction Electrolysis is the process in which an electric current produces a chemical reaction. Electrolysis Setup Diagram. What happens during electrolysis of salt water with copper electrodes? You used a copper electrode at the anode and a leaf covered in graphite powder as the cathode in a copper sulphate solution. This example appears as an answer to another question in Quora. Platinum anodes were not inert at certain combinations of temperature and current density, and platinum acted as a low overvoltage impurity. 999 percent is not unusual. 3 Deduce from 1 and 2 the charge required to remove one mole of. Write the reduction reaction equation for the production of copper metal from molten copper sulfate: Cu2+ + 2e. Copper(II) ions are deposited as copper on the cathode (for the electrode equation, see under the purification of copper below). 5 Do not write outside the box (05) G/Jun17/CH2FP Turn over 2 This question is about sulfuric acid, copper sulfate and ethene. During the electrolysis of copper (II) sulfate, or #"CuSO"_4"#, the deposition of copper can be seen on the cathode; at the same time, the anode will be dissolved by the process. Write the full name of elements in copper sulphate and radicals followed by its symbols and write a balanced equation for electrolysis of water balance the equation. Electrolysis has many practical and industrial applications. This implies to me that both nitrites are formed as side reactions to the presence of NO and NO2 gases (and NH3 per equation [1] above in the formation of NH4NO2). Naked Science Forum King! 7813;. Electrolysis of copper (II) sulphate solution using copper electrodes Apparatus and chemicals: Copper foils as electrodes, copper(II) sulphate solution, Dry cells or car battery. Colourless gas bubbles are released. A copper wire was placed in a 600 mL beaker with the wire extending from the beaker. Electrolysis of copper sulfate: Two copper electrodes are placed in a solution of blue copper sulfate and are connected to a source of electrical current. Write equations for the anode and cathode reactions. Two graphite electrodes were connected to a D. So it can be concluded that, during electrolysis of copper sulfate with copper electrodes. Calculate the concentration of copper sulphate in the solution to begin with. Copper can be produced from copper(II) sulfate solution by two different methods. Include cell diagram, observations, anode and cathode reactions and state the uses. 65 x 104C) 63. (a) A student was given two different types of electrodes (carbon and copper electrodes) to carry out electrolysis of copper(II) sulfate solution. It was found that after electrolysis the absorbance of the solution was reduced to 50 % of its original value. This example appears as an answer to another question in Quora. We measure the distance between adjacent trees, calculate. The item will become coated in copper. 403 V (see equations c and b, above) , it breaks the thermodynamic requirement of 1. Begins with a starter activity to get students thinking about ion present in ionic compounds then focuses of aqueous copper (II) sulfate. Electrolytic processes. In this process, the positive electrode (the anode) is made of the impure copper which is to be purified. Write the reduction reaction equation for the production of copper metal from molten copper sulfate:. (c) Calcium nitrate reacts with sodium sulphate to form calcium sulphate (same is required in two places). Copper ions and sulfate ions. The method used to extract a metal from its ore is linked to the reactivity of the metal. and S0 42- migrate to the anode, but none of them get discharged because the copper of the anode dissolves in the solution. Electrolysis. Study Electrolysis Experperiment 1 (Sodium Sulfate Solution) flashcards from Cathal O'Leary's class online, or in Brainscape's iPhone or Android app. Copper sulphate solution (250 ml) was electrolysed using a platinum anode and a copper cathode. This is a non-spontaneous reaction. •Electrolysis •Electrolysis of salts •Uses of electrolysis Write balanced half equations for the reaction at the anode or cathode for Na+ ions , Pb2+, Br- and Cl-ions. A mixture of magnesium sulfate and zinc nitrate with graphite electrodes. In order to electrolyze water , a little amount of an electrolyte (salt or acid) is added to water, which makes it an electrolyte. Cathode: Cu (s) → Cu 2+ (aq) + 2e -. which indicates that the zinc reacts with the copper sulphate solution to produce copper and zinc sulphate solution. Write equations for the reactions taking place at the two electrodes (mentioning clearly the name of the electrode) during the electrolysis of : (i) Acidified copper sulphate solution with copper electrodes. Both forms are incompatible with finely powdered metals. electrolysis o f water Water is a weak electrolyte because it conducts very little amount of electric current. 2a and 2b show the kinetic results of copper electrodeposition (i. Anode (+) Cathode (-) Ion presents. A direct electric current is passed through the solution. Electrolysis is also used in electroplating. Electrolysis. During the electrolysis of Aqueous Copper(II) Sulfate with inert electrodes what is formed at the anode and what is the half equation? Water and Oxygen, 4OH⁻ → O₂ + 2H₂O + 4e⁻ During the electrolysis of Dilute Sulfuric Acid with inert electrodes what is formed at the cathode and what is the half equation?. Copper(II) ions are deposited as copper on the cathode (for the electrode equation, see under the purification of copper below). Why does the colour of copper sulphate solution change when an iron nail is dipped in it? Write two observations. wikiHow is a “wiki,” similar to Wikipedia, which means that many of our articles are co-written by multiple authors. This article has also been viewed 167,990 times. !Copper is extracted from copper sulfide. The reaction at the cathode: Cu++(aq) plus 2e- = Cu(s). 55: Write ionic half-equations representing the reactions at the electrodes during electrolysis December 27, 2016; 1. During the electrolysis of …. Example 2 - Electrorefining of copper. At the cathode: Copper(II) ions are reduced to form copper metal, which is deposited on the object. Thus, in the electrolysis of fused magnesium chloride, MgCl 2, one faraday of electricity will deposit 24. (a) The electrolysis of lead bromide liberates lead and bromine. CH 302 13 Answer Key More Advanced Electrochemistry Problems 1. Extraction of Metals. - Electrolysis Investigation To monitor the quantity of copper (Cu) metal deposited during the electrolysis of copper sulphate solution. Revision Notes 6. I chose the Copper Sulfate Electrolyte, a Copper Anode, a Steel Cathode and a Battery as the components in the illustration of a circuit on Electroplating. Give a method for making copper sulfate crystals from copper oxide and dilute. 4 the purification of copper using aqueous copper(II) sulfate. During the electrolysis process, copper atoms leave the copper sulfate solution and form a coating on the anode, leaving sulfur residue in the electrolytic solution. Which products form in the electrolysis of sodium chloride solution? Which products form in the electrolysis of : (i) Copper chloride solution (ii) copper sulfate solution. Observation. the electrode connected to the negative terminal of the battery. CONCEPT DIAGRAM. + + (cation) and SO. 022 x 10 23 words. - Each zinc atom transferred two electrons directly to a copper (II) ion in this redox reaction. First, he carried out the experiment with carbon electrodes. Electrolysis of the ionic compound Sodium Chloride is commonly carried out to obtain Sodium metal.
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