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NEET · Chemistry · STD 12 - 3. Chemical kinetics
For a reaction, activation energy \(\mathrm{E}_{\mathrm{a}}=0\) and the rate constant at \(200\; \mathrm{K}\) is \(1.6 \times 10^{6} \;\mathrm{s}^{-1} .\) The rate constant at \(400\; \mathrm{K}\) will be glven that gas constant] \(\mathrm{R}=8.314\; \mathrm{JK}^{-1} \mathrm{mol}^{-1}\)
- A \(3.2\times 10^{4} \;\mathrm{s}^{-1}\)
- B \(1.6\times 10^{6} \;\mathrm{s}^{-1}\)
- C \(1.6\times 10^{3} \;\mathrm{s}^{-1}\)
- D \(3.2 \times 10^{6} \;\mathrm{s}^{-1}\)
Answer & Solution
Correct Answer
(B) \(1.6\times 10^{6} \;\mathrm{s}^{-1}\)
Step-by-step Solution
Detailed explanation
\(\log \left(\frac{\mathrm{K}_{2}}{\mathrm{K}_{1}}\right)=\frac{\mathrm{E}_{\mathrm{a}}}{2.303 \mathrm{R}}\left(\frac{1}{\mathrm{T}_{1}}-\frac{1}{\mathrm{T}_{2}}\right)\) \(\mathrm{E_a}=0\)
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