where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as follows: Ag+(aq) + e– --> Ag(s); Eo = 0.80 V Ni2+(aq) + 2e– --> Ni(s); Eo = – 0.23 V What is the Ecell at 25oC when the electrolyte concentrations are: [Ag+] = 1.3 x 10–5 M and [Ni2+] = 0.10 M.

where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as follows: Ag+(aq) + e– --> Ag(s); Eo = 0.80 V Ni2+(aq) + 2e– --> Ni(s); Eo = – 0.23 V What is the Ecell at 25oC when the electrolyte concentrations are: [Ag+] = 1.3 x 10–5 M and [Ni2+] = 0.10 M.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 95QRT

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Concept explainers

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.

Question

100%

Consider the same diagram of a galvanic cell as in previous question,

where the half-cells are Ag|AgNO₃(aq) and Ni|Ni(NO₃)₂(aq), and the electrode potentials are as follows:

Ag⁺(aq) + e^– --> Ag(s); E^o = 0.80 V

Ni²⁺(aq) + 2e^– --> Ni(s); E^o = – 0.23 V

What is the E_cell at 25^oC when the electrolyte concentrations are: [Ag⁺] = 1.3 x 10^–⁵ M and [Ni²⁺] = 0.10 M.

(A) 1.15 V

(B) 1.30 V

(D) 0.91 V

conventional current
A
e flow
+
Salt bridge
anode
• cathode
X*(aq)
Y*(aq)

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