JEE Mains · Chemistry · STD 12 - 3. Chemical kinetics
Consider the two different first order reactions given below \(\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}\) (Reaction 1\()\) \(\mathrm{P} \rightarrow \mathrm{Q}\) (Reaction \(2\)) The ratio of the half life of Reaction \(1\) : Reaction \(2\) is \(5: 2\). If \(t_1\) and \(t_2\) represent the time taken to complete \(2 / 3^{\text {dd }}\) and \(4 / 5^{\text {dd }}\) of Reaction \(1\) and Reaction \(2\), respectively, then the value of the ratio \(\mathrm{t}_1: \mathrm{t}_2\) is _______ \(\times 10^{-1}\) (nearest integer). [Given: \(\log _{10}(3)=0.477\) and \(\log _{10}(5)=0.699\) ]
- A \(15\)
- B \(18\)
- C \(20\)
- D \(17\)
Answer & Solution
Correct Answer
(D) \(17\)
Step-by-step Solution
Detailed explanation
\(\frac{\left(\mathrm{t}_{1 / 2}\right)_{\mathrm{I}}}{\left(\mathrm{t}_{1 / 2}\right)_{\mathrm{II}}}=\frac{\mathrm{K}_2}{\mathrm{~K}_1}=\frac{5}{2}\) \(\therefore \mathrm{K}_1 \mathrm{t}_1=\ln \frac{1}{1-\frac{2}{3}}=\ln 3\)…
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