Difficult
For the hypothetical reaction $2X + G \to Q + 2M$,the rate expression is $\frac{d[Q]}{dt} = k[X]^2$. Which of the following is the most likely mechanism?
- A$2X + G \rightleftharpoons 2Q + R$ (fast)
$Q + R + G \to 2M$ (slow) - B$X + G \rightleftharpoons Q + R$ (fast)
$R + X \to 2M$ (slow) - C$X + X \rightleftharpoons X_2$ (fast)
$X_2 \to Q + T$ (slow)
$T + G \to 2M$ (fast) - D$G + G \rightleftharpoons G_2$ (fast)
$G_2 + X \to Q + T$ (slow)
$T + X \to 2M$ (fast)
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Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$
takes place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{slow} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{fast} H_2O + Br_2$
The order of the reaction is
takes place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{slow} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{fast} H_2O + Br_2$
The order of the reaction is
Difficult
View SolutionThe rate of a gaseous reaction is given by the expression $K [A] [B]$. If the volume of the reaction vessel is suddenly reduced to $1/4$ of the initial volume,the reaction rate relating to the original rate will be
Medium
View SolutionThe initial rates of decrease of $I_2$ in acetone-iodine reaction catalysed by $H^{+}$ are given in the table.
Experiment Initial $[I_2]$ $(mol \ L^{-1})$ Initial $[H^{+}]$ $(mol \ L^{-1})$ Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$ Initial rate $(mol \ L^{-1} \ s^{-1})$ $1$ $0.01$ $0.1$ $0.1$ $0.096$ $2$ $0.01$ $0.2$ $0.1$ $0.192$ $3$ $0.02$ $0.2$ $0.1$ $0.192$ $4$ $0.01$ $0.2$ $0.2$ $0.384$
The order with respect to $I_2, H^{+}$,acetone and total order of the reaction respectively are:
| Experiment | Initial $[I_2]$ $(mol \ L^{-1})$ | Initial $[H^{+}]$ $(mol \ L^{-1})$ | Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$ | Initial rate $(mol \ L^{-1} \ s^{-1})$ |
| $1$ | $0.01$ | $0.1$ | $0.1$ | $0.096$ |
| $2$ | $0.01$ | $0.2$ | $0.1$ | $0.192$ |
| $3$ | $0.02$ | $0.2$ | $0.1$ | $0.192$ |
| $4$ | $0.01$ | $0.2$ | $0.2$ | $0.384$ |
The order with respect to $I_2, H^{+}$,acetone and total order of the reaction respectively are:
For the reaction $2A + B \rightarrow \text{Product}$,the rate constant $(K)$ is $2.5 \times 10^{-5} \text{ L mol}^{-1} \text{ s}^{-1}$ after $15 \text{ s}$,$2.60 \times 10^{-5} \text{ L mol}^{-1} \text{ s}^{-1}$ after $30 \text{ s}$,and $2.55 \times 10^{-5} \text{ L mol}^{-1} \text{ s}^{-1}$ after $50 \text{ s}$. What is the order of the reaction?
Medium
View SolutionThe temperature coefficient of most reactions lies between $.......$.
Medium
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