Medium
If a reaction has the experimental rate expression $\text{rate} = K [A]^2[B]$,what happens to the reaction rate if the concentration of $A$ is doubled and the concentration of $B$ is halved?
- ARate becomes double
- BRate becomes eight times
- CRate becomes tripled
- DNo change in rate
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The results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
Experiment $[A] / mol \ L^{-1}$ $[B] / mol \ L^{-1}$ Initial rate / $mol \ L^{-1} \ min^{-1}$ $I$ $0.1$ $0.1$ $6.00 \times 10^{-3}$ $II$ $0.1$ $0.2$ $2.40 \times 10^{-2}$ $III$ $0.2$ $0.1$ $1.20 \times 10^{-2}$ $IV$ $X$ $0.2$ $7.20 \times 10^{-2}$ $V$ $0.3$ $Y$ $2.88 \times 10^{-1}$
$X$ and $Y$ in the given table are respectively :
$2 A + B \longrightarrow C + D$
| Experiment | $[A] / mol \ L^{-1}$ | $[B] / mol \ L^{-1}$ | Initial rate / $mol \ L^{-1} \ min^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $6.00 \times 10^{-3}$ |
| $II$ | $0.1$ | $0.2$ | $2.40 \times 10^{-2}$ |
| $III$ | $0.2$ | $0.1$ | $1.20 \times 10^{-2}$ |
| $IV$ | $X$ | $0.2$ | $7.20 \times 10^{-2}$ |
| $V$ | $0.3$ | $Y$ | $2.88 \times 10^{-1}$ |
$X$ and $Y$ in the given table are respectively :
DifficultJEE MAIN 2020
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Medium
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