Consider a voltaic cell that operates using the following redox reaction:
Ni²⁺ (aq) + Co (s) →Ni (s) + Co²⁺ (aq) E ° _cell = 0.03 V What is the cell potential, E _cell, at 298 K under non-standard conditions when [Ni²⁺] = 0.80 M and [Co²⁺] = 0.20 M?

Question

Quizplus · Accepted Answer

The cell potential, E _cell, under non-standard conditions can be calculated using the Nernst equation: E _cell = E ° _cell - (0.0592 V / n) log Q, where Q is the reaction quotient and n is the number of electrons transferred in the reaction. First, we need to write the balanced equation for the reaction: Ni²⁺ (aq) + Co (s) → Ni (s) + Co²⁺ (aq) The number of electrons transferred in the reaction is 1. The reaction quotient is: Q = ([Ni]/[Co]) = (0.80 M / 0.20 M) = 4 Substituting in these values, we get: E _cell = 0.03 V - (0.0592 V / 1) log 4 E _cell = 0.03 V - 0.057 V E _cell = 0.048 V Therefore, the correct answer is (C).

Consider a Voltaic Cell That Operates Using the Following Redox