Author Question: A strip of copper is placed in a 1 M solution of copper nitrate and a strip of silver is placed in a ... (Read 158 times)

Deast7027 · **on:** Mar 21, 2021

Question 1

A solution of MnO₄^2– is electrolytically reduced to Mn³⁺. A current of 5.29 amp is passed through the solution for 15.0 minutes. What is the number of moles of Mn³⁺ produced in this process? (1 faraday = 96,485 coulombs)

◦ 0.0493 mol
◦ 0.148 mol
◦ 2.74 × 10^–4 mol

◦ 0.0164 mol
◦ 1.10 × 10^–3 mol

Question 2

A strip of copper is placed in a 1 M solution of copper nitrate and a strip of silver is placed in a 1 M solution of silver nitrate. The two metal strips are connected to a voltmeter by wires and a salt bridge connects the solutions. The following standard reduction potentials apply:

	Ag⁺(aq) + e^– Ag(s)	E° = +0.80 V
	Cu²⁺(aq) + 2e^– Cu(s)	E° = +0.34 V

Which of the following statements is false?

◦ Electrons flow in the external circuit from the copper electrode to the silver electrode.
◦ The silver electrode increases in mass as the cell operates.
◦ There is a net general movement of silver ions through the salt bridge to the copper half-cell.
◦ Negative ions pass through the salt bridge from the silver half-cell to the copper half-cell.
◦ Some positive copper ions pass through the salt bridge from the copper half-cell to the silver half-cell.

micaelaswann · **Reply #1 on:** Mar 21, 2021

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