How many minutes are required to deposit 2.73 g Cr from a Cr³⁺(aq) solution using a current of 2.50 A? (F = 96,500 C/mol)

Q: How many grams of Pb would be deposited from an aqueous solution of Pb 2+ with a current of 1.828 A…

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Q: A current of 3.12 A3.12 A is passed through a Sn(NO3)2Sn(NO3)2 solution for 1.20 h1.20 h. How much…

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Q: How many minutes will it take for a current of 10.4 A to deposit 4.06 g of gold from a solution of…

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Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: EFM of the cell is calculated by using below formula,

Q: A current of 4.76 A is passed through a Fe(NO3)2 solution for 1.20 h. Calculate the charge that…

A: Current = 4.76 A Time = 1.20 h

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: How many minutes are required to deposit 2.28 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: Faraday's Law of Electrolysis: According to this law during electrolysis, the amount of chemical…

Q: How many minutes are required to deposit 1.39 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

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Q: How many grams of copper metal can be deposited from Cu2*(aq) when a current of 2.50 A is run for…

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Q: A tub of water containing Cr³⁺(aq) is subjected to a current of 1.0 amperes for 60 minutes. How many…

A: An external source of voltage is used to carry out a reaction in case of electrochemical cell. The…

Q: How many minutes are required to deposit 1.42 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: Given:  W = 1.42 gm  I = 2.50 A  Mol. Wt. of Cr = 52  'n' factor of Cr = 3  Equivalent wt. of Cr =…

Q: How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn2+ (s the solution…

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Q: Determine the current (in A) to produce 6.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: Given information  Mass of Ag = 6.50 g Time = 2.00 h To calculate: Current

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2*(aq)…

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Q: Determine the current (in A) to produce 3.10 g Ag when Ag"(aq) is electrolyzed for 2.00 h. (F =…

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Q: 9. A concentrated Pb(NO3)2 (aq) solution is electrolyzed using a current of 10.5 A. a) What mass of…

A: SOLUTION: Step 1: Hello. Since the question contain multiple sub-parts, the first three subparts are…

Q: A current of 4.15 A is passed through a Pb(NO3)2 solution for 1.50 h. How much lead is plated out of…

A: Given that:  Current(I) = 4.15A = 4.15C/s  Time(t) = 1.50h = 1.50h×3600s/h = 5400s Reaction:  Pb2+ +…

Q: A current of 5.83 A is passed through a Fe(NO3)2 solution for 1.60 h. How much iron is plated out of…

A: According to Faraday's law of electrolysis, the amount of substance deposited on an electrode is…

Q: 3. How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn²+ (aq) if the…

A:

Q: Determine the current (in A) to produce 4.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

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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 current of 4.30 A is passed through a Pb(NO3)2 solution for 1.80 h. How much lead is plated out of…

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Q: Calculate the mass in grams of a metal Q ( Molar mass= 88.23 g/mol) that will be deposited from a…

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Q: How many minutes are required to deposit 1.48 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: According to Faraday's law of electrolysis, the mass (m) of substance deposited at the electrode is…

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: Given, Current deposited = 2.50  Time = 2.95 h F = 96500 C/mol

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: By using Faraday law, we can find mass of Cu deposited at respective electrode.   The following…

Q: How many grams of Ag would be deposited from an aqueous solution of Ag+ with a current of 2.534 A…

A: Molar mass of Ag = 108g/mol Reaction takes place:- Ag+ + e-  ------> Ag  current , I = 2.534 A…

Q: How many seconds are required to deposit 0.145 grams of zinc metal from a solution that contains Zn*…

A: Answer :-  t = 447 (s) The time required to deposit 0.145 g of Zn metal from a Zn2+ solution when…

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

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Q: How many grams of silver metal are produced from Ag⁺(aq) in 5.25 h with a current of 3.50 A? (F =…

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Q: Cr3+(aq)Cr3+(aq) solution is electrolyzed using a current of 7.80 AA.     Part A What mass of…

A: Part A :  current passed through solution = 7.80 A  Time = 3.00 days  Since 1 day = 86400 sec  =>…

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: As per the given information  current =2.50 A Time = 5.30 hours or  The calculation of amount of…

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: How many grams of silver metal are produced from Ag⁺(aq) in 1.25 h with a current of 3.50 A? (F =…

A: Interpretation-  To determine the grams of silver metal produced from Ag+ (aq) in 1.25h with a…

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.