Chemistry-Nernst Equation

NEET Chemistry Nernst Equation MCQ Question

Type: MCQ-numerical-Hard-Class 12

Calculate the cell potential EcellE_{\text{cell}} at 298 K for the cell reaction Ni(s) + 2Ag^+(0.010 M) \rightarrow Ni^{2+}(0.100 M) + 2Ag(s) giventhestandardcellpotentialgiven the standard cell potential E^o_{\text{cell}} = 1.05, V $. Use the Nernst equation to find the answer.

A

0.91 V

B

05 V

C

19 V

D

0.78 V

Correct Answer

Option A

Detailed Explanation

Using the Nernst equation Ecell=EcelloRTnFlnQE_{\text{cell}} = E^o_{\text{cell}} - \frac{RT}{nF} \ln Q, where Q=[Ni2+][Ag+]2Q = \frac{[Ni^{2+}]}{[Ag^+]^2}, we calculate Ecell=1.050.0592ln0.100(0.010)2E_{\text{cell}} = 1.05 - \frac{0.059}{2} \ln \frac{0.100}{(0.010)^2}, resulting in a potential of 0.91 V.

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