The rate of reaction,$A + B \rightarrow \text{product}$,is $7.2 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ at $[A] = 0.4 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$. The reaction is first order in $A$ and second order in $B$. Calculate the rate constant.
- A$14 \ mol^{-2} \ dm^6 \ s^{-1}$
- B$12 \ mol^{-2} \ dm^6 \ s^{-1}$
- C$18 \ mol^{-2} \ dm^6 \ s^{-1}$
- D$20 \ mol^{-2} \ dm^6 \ s^{-1}$
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Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
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$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
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$(iii)$ $X + Y \rightarrow XY$ (fast)
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