Example 9. In an electrolysis experiment, a current was passed for 5 hours through two cells connected in series. The first cell contains a solution of gold salt and the second cell contains copper sulphate solution. 9.85 g of gold was deposited in the first cell. If the oxidation number of gold is +3, find the amount of cop- per deposited on the cathode in the second cell. Also, calculate the magnitude of the current in ampere.

Q: Complete the following on paper, SHOWING ALL WORK. Al3+ is reduced to Al(s) at an electrode. If a…

A: As per the question balance chemical equation is as follows:         Current (I)= 2.00 ampere…

Q: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

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Q: A certain half-reaction has a standard reduction potential End=+0.27 V. An engineer proposes using…

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Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

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Q: A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

A: Given : Current = 7.1 A And time = 40 min = 40 X 60 = 2400 s…

Q: A certain half-reaction has a standard reduction potential Ed=+0.73 V. An engineer proposes using…

A: Given,The standard reduction potential: , this is the reduction potential of the anode.Also,  (at…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: left half cell concentration = 3.00MRight half cell concentration = 15mMTemperature T= C + 274 =…

Q: Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate…

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Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

Q: A certain half-reaction has a standard reduction potential Ered =-0.96 V. An engineer proposes using…

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Q: A constant current of 0.712 A is passed through an electrolytic cell containing molten BaCl2 for…

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Q: A factory wants to produce 1.00 x 103 kg barium from the electrolysis of molten barium chloride.…

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Q: A constant current of 0.445 A is passed through an electrolytic cell containing molten BaCl2 for…

A: The reaction is, Ba2+ + 2e- ---> Ba(s) From this reaction, we can conclude that 2 mol of…

Q: n a copper plating experiment in which copper metal is deposited from a copper(II) ion solution, the…

A: Using Faraday's First of electrolysis: w = ZIt Z = Equivalent mass of metal96500w = Molar mass of Cu…

Q: A certain half-reaction has a standard reduction potential Ered = +0.73 V. An engineer proposes…

A: Ecello=1.00 VEcathodeo= +0.73 V

Q: What current must be supplied to deposit 4.77 g of gold from a solution of AuCl 3 in 27.2 min?

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Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

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Q: In one process used for electroplating silver, a current of 10.23 A was passed through an…

A: Dear student, this question is related to electroplating process.

Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

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Q: Two electrolytic cells are connected in series. The 1st cell contains copper sulfate solution while…

A: Given the current supplied to both the electrodes, I = 0.5 A Given the Ag electrode has 0.2 g lesser…

Q: What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given ,

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: How long ( hours) would it take to unload 0.433 moles of vibranium (Vb) metal during electrolysis of…

A: We have to calculate time needed for electrolysis  Molar mass of Tr not provided so only 1st…

Q: Electrolysis can be used to purify silver.  What mass of silver would plate onto the pure electrode…

A: One Mole of electron = 96500 C

Q: A current of 5.55 A is passed through a Cu(NO3)2 solution for 1.90 h. How much copper is plated out…

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Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

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Q: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

Q: A certain half-reaction has a standard reduction potential -0.64 v. An engineer proposes using this…

A: Given:  (E°reduction)anode = -0.64 V  E°cell = 0.90 V

Q: 4. (10 points) An electrolytic cell is set up with a metal object to be electroplated by the…

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Q: A1.0-L sample of 1.0 M HCI solution has a 13.5 A current applied for 41 minutes. What is the pH of…

A: Since HCl is a strong acid. Hence it will dissociate completely into ions Hence moles of HCl = moles…

Q: A current was passed for 5 hours through two electrolytic cells connected in series. The first cell…

A: Chemical equations for the reduction of gold and copper ions are: Au3+(aq)+3e-→Au(s)…

Q: A factory wants to produce 1.00 x 103 kg barium from the electrolysis of molten barium chloride.…

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Q: A current of 0.44A is passed through a solution of ruthenium nitrate causing reduction of the metal…

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.