VOLTAIC CELL AND ELECTROLYSIS1. Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic cellexperiment on an unknown metal solution. She was able to deposit 9.701 g of the metal as solid on thecathode after applying a 1.500 A current for 10.00 hours. Her assistant, Oz, had previously noted that 3electrons are involved per mole of the metal deposited.a. Determine the molar mass of the unknown metal in g/mol.g/molb. What is the identity of the unknown metal?MnCd| Cripts of the compounds or ions, the text formatting isSrgiven as follows:Cd2+ = Cd^2+Cu2+ = Cu^2+2. In another experiment, Fischl used cadmium metal to form an electrode she can use for her voltaic cell.She wanted to determine the electric potential produced by the cadmium electrode (and 1.0 M of itscorresponding electrolyte solution) with a Copper electrode in 0.10 M CuSO4 solution at 25 °C. Predict thefollowing:a. OHR of the voltaic cell:Cd^2+(aq)+ 2e- → Cd(s), Eo = - 0.40 VCu^2+(aq) + 2e- → Cu(s), Eo = + 0.34 VCu(s) → Cu^2+(aq)+ 2e-, Eo = - 0.34 VCd(s) → Cd^2+(aq)+ 2e-, Eo = + 0.40 Vb. RHR of the voltaic cell:Cu(s) → Cu^2+(aq)+ 2e-, Eo = - 0.34 VCd^2+(aq)+ 2e- → Cd(s), Eo = - 0.40 VCu^2+(aq) + 2e- → Cu(s), Eo = + 0.34 VCd(s) → Cd^2+(aq)+ 2e-, Eo = + 0.40 Vc. Number of electrons involved in the redox reaction (n):d. Overall reaction for the voltaic cell:e. Standard cell potential, E°cell:Vf. Theoretical Ecell :Vg. If the measured Ecell was 0.50 V, calculate the percent error.

Since you have asked multiple question, we will solve the first question for you. If you want any…

VOLTAIC CELL AND ELECTROLYSIS 1. Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic cell experiment on an unknown metal solution. She was able to deposit 9.701 g of the metal as solid on the cathode after applying a 1.500 A current for 10.00 hours. Her assistant, Oz, had previously noted that 3 electrons are involved per mole of the metal deposited. a. Determine the molar mass of the unknown metal in g/mol. g/mol b. What is the identity of the unknown metal? Mn Cd | Cr ipts of the compounds or ions, the text formatting is Sr given as follows: Cd2* = Cd^2+ Cu2+ = Cu^2+

VOLTAIC CELL AND ELECTROLYSIS 1. Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic cell experiment on an unknown metal solution. She was able to deposit 9.701 g of the metal as solid on the cathode after applying a 1.500 A current for 10.00 hours. Her assistant, Oz, had previously noted that 3 electrons are involved per mole of the metal deposited. a. Determine the molar mass of the unknown metal in g/mol. g/mol b. What is the identity of the unknown metal? Mn Cd | Cr ipts of the compounds or ions, the text formatting is Sr given as follows: Cd2* = Cd^2+ Cu2+ = Cu^2+

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 76AP

See similar textbooks

Similar questions

A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
Consider a galvanic cell based on the following half-reactions: a. What is the standard potential for this cell? b. A nonstandard cell is set up at 25C with [Mg2+] = 1.00 105 M. The cell potential is observed to be 4.01 V. Calculate [Au3+] in this cell.