NEET Chemistry Nernst Equation MCQ Question with Solution

Calculate the cell potential $E_{\text{cell}}$ at 298 K for the cell reaction Ni(s) + 2Ag^+(0.010 M) \rightarrow Ni^{2+}(0.100 M) + 2Ag(s) $given the standard cell potential$ 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 $E_{\text{cell}} = E^o_{\text{cell}} - \frac{RT}{nF} \ln Q$ , where $Q = \frac{[Ni^{2+}]}{[Ag^+]^2}$ , we calculate $E_{\text{cell}} = 1.05 - \frac{0.059}{2} \ln \frac{0.100}{(0.010)^2}$ , resulting in a potential of 0.91 V.

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NEET Chemistry Nernst Equation MCQ Question

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