Calculate the mass of silver deposited at the cathode during electrolysis when a current of 1.80A flows through an aqueous solution of silver nitrate for 45.0 min. (A, value: [Ag] = 108; F = 96500 C mol-1)

Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

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Q: A constant current of 1.6 A is used to precipitate copper at the cathode and oxygen at the anode of…

A: value of constant current = 1.6 A Time = 30.4 minutes cathode - copper Anode - oxygen

Q: How many seconds are required to deposit 0.189 grams of manganese metal from a solution that…

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Q: How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through…

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Q: 4. A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x…

A: Given current = 7 A standard value  density of gold = 19.3 g/cm3

Q: A molten binary salt, Cal2, is electrolyzed. Write the half reactions that occur and identify which…

A: The binary salt given is CaI2  hence it has cation Ca2+ and anions I-

Q: Determine the molar mass (amu) of Metal (M) if it took 2.05 minutes for a current of 1.91 A to plate…

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Q: The passage of a current of 0.750 A for 25.0min deposited 0.369 g of copper from a CuSO4 solution.…

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Q: How much time in minutes would it take to deposit 4.01 grams of X (MW 163.10 g/mol) on a cathode in…

A: Faraday's second law states that, the amount of substances deposited by the passage of same amount…

Q: How many seconds are required to deposit 0.268 grams of iron metal from a solution that contains…

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Q: In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode. Using…

A: (a) Current is the amount of charge flowing per unit time. If I is the current(in A) andt is the…

Q: A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5in x 8.5in x…

A: first we have to find the volume,volume=length ×width×heightthen we know,density=massvolumeby…

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

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Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

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Q: What mass of copper , in mg , can be deposited from copper (II) sulfate solution using a current of…

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Q: If a water electrolysis cell operates at a current of 7.8 A, how longwill it take to generate 25.0 L…

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

A: Given: Current = 2.96 A Time = 33.4 min Mass of V deposited at cathode = 0.784 g Molar mass of V =…

Q: Molten AlCl3 is electrolyzed for 5.0 hours with a current of 0.40amperes.  metallic aluminum is…

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Q: A galvanic cell is constructed with a silver-silver chloride electrode, and a nickel strip immersed…

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Q: A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

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Q: Identify the reaction that occurs at the anode and the cathode. anode: cathode: Determine the…

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Q: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: How long will it take to deposit 1.5 g of Cu on a metal when a current of 5 A is applied to a CuSO4…

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Q: Calculate the minimum voltage in volts required to drive the electrolysis reaction of molten LiCl by…

A: The half-cell reactions are: Anode: Li(s) -----> Li+ + e- Eº = -3.03V Cathode: Cl2 + 2e-…

Q: How many seconds are required to deposit 0.270 grams of copper metal from a solution that contains…

A: Given weight of deposited copper metal from a solution(w) = 0.270 g  Current applied (I)= 0.828 A =…

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Current = 5 A Voltage = 4.5 V Time = ? Volume = 215 mL = 0.215 L Molarity = 1.19 M

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Q: Calculate the time to deposit 1.5 g of silver at cathode when a current of 1.5 A was passed through…

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

A: Current I = 1.46 A  time t = 23.1 minutes = 23.1 * 60 s = 1386 s Mass of vanadium deposited = 0.534…

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

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Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

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Q: A solution of CuSO4 is electrolysis for 10 minutes with a current of 1.5 amperes. What is the mass…

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Q: During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on…

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Q: If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how…

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Q: How many grams of  zinc metal will be deposited from a solution that contains  Zn^2+ ions if a…

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Q: A Galvanic cell is consisting of standard concentrations: Cu|Cu2+||Ag+ |Ag, is connected to a small…

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Q: In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode. Using…

A: Given,  Current in ampere = I =  0.150 A  Electrolysis of Ni2+ (aq) ion  Time period in minutes = t…

Q: A steady current of 5 A is maintained for 120 seconds in CUSO4 solution. How much Cu is deposited in…

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Q: The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a CuSO, solution.…

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Q: In the electrolysis of a solution containing Ag* (aq), metallic Ag(s) deposits on the cathode. Using…

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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.