Medium
Which of the following statements is $NOT$ true for a reaction having rate law $r=k[H_2][I_2]$?
- AThe reaction is first order in $H_2$
- BOverall order of reaction is $1$
- CThe reaction is first order in $I_2$
- DOverall order of reaction is $2$
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Consider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:
$[A_2]_0$ $[B_2]_0$ Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ $0.1 \ M$ $0.1 \ M$ $2.5 \times 10^{-4}$ $0.2 \ M$ $0.1 \ M$ $5.0 \times 10^{-4}$ $0.2 \ M$ $0.2 \ M$ $1.0 \times 10^{-3}$
The value of the rate constant for the above reaction is:
| $[A_2]_0$ | $[B_2]_0$ | Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $2.5 \times 10^{-4}$ |
| $0.2 \ M$ | $0.1 \ M$ | $5.0 \times 10^{-4}$ |
| $0.2 \ M$ | $0.2 \ M$ | $1.0 \times 10^{-3}$ |
The value of the rate constant for the above reaction is:
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