Back to Practice
AIIMS2019Chemistry-Electrochemistry

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.

Found an issue with this question?

Related Questions

Explore More Questions

All Chemistry QuestionsElectrochemistry QuestionsAIIMS 2019 PYQ