WBJEE · Chemistry · Chemical Kinetics
Consider the following two first order reactions occurring at 298 K with same initial concentration of \(A\) :(1) \(A \rightarrow B ;\) rate constant, \(k=0.693 \mathrm{min}^{-1}\) (2) \(A \rightarrow C\); half-life, \(l_{1 / 2}=0.693\) min Choose the correct option.
- A Reaction (1) is faster than reaction (2).
- B Reaction (1) is slower than reaction (2).
- C Both reactions proceed at the same rate.
- D Since two different products are formed, rates cannot be compared.
Answer & Solution
Correct Answer
(B) Reaction (1) is slower than reaction (2).
Step-by-step Solution
Detailed explanation
Given, for two first order reactions. \[ A \rightarrow B k=0.693 \mathrm{min}^{-1}...(1) \] and \[ A \rightarrow C, t_{1 / 2}=0.693 \mathrm{min}...(2) \] For first order reaction \[ t_{1 / 2}=\frac{0.693}{k} \] Thus, for the reaction \(A \rightarrow B\)…
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