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AIIMS 2019 Chemistry Nernst Equation MCQ Question

Type: MCQ-conceptual-Medium-Class 12

The decomposition of NH3\text{NH}_3 on Pt surface is a zero order reaction. If the value of rate constant is 2×10−4 mole liter−1 sec−12 \times 10^{-4} \text{ mole liter}^{-1} \text{ sec}^{-1}. The rate of appearance of N2\text{N}_2 and H2\text{H}_2 are respectively.

A

1×10−4 mol l−1 sec−1, 3×10−4 mol l−1 sec−11 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1} \text{, } 3 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1}

B

3×10−4 mol l−1 sec−1, 1×10−4 mol l−1 sec−13 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1} \text{, } 1 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1}

C

2×10−4 mol l−1 sec−1, 6×10−4 mol l−1 sec−12 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1} \text{, } 6 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1}

D

3×10−4 mol l−1 sec−1, 3×10−4 mol l−1 sec−13 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1} \text{, } 3 \times 10^{-4} \text{ mol l}^{-1} \text{ sec}^{-1}

Correct Answer

Option C

Detailed Explanation

The calculation of the standard reduction potential EH2/H+E_{H_2/H^+} using the Nernst equation shows that at a pH of 10, the concentration of [H+][H^+] is 10−10 M10^{-10} \, \text{M}. Substituting this value into the Nernst equation yields EH2/H+=0−0.0592log⁡((10−10)21)=0.59 VE_{H_2/H^+} = 0 - \frac{0.059}{2} \log \left(\frac{(10^{-10})^2}{1}\right) = 0.59 \, \text{V}, confirming that option C is correct. Other options are not applicable as they do not provide relevant information or calculations related to the Nernst equation or the given reaction.

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