Difficult
Consider the following data for the given reaction $2 HI_{(g)} \rightarrow H_{2_{(g)}} + I_{2_{(g)}}$. The order of the reaction is:
Experiment $1$ $2$ $3$ $[HI] \ (mol \ L^{-1})$ $0.005$ $0.01$ $0.02$ Rate $(mol \ L^{-1} \ s^{-1})$ $7.5 \times 10^{-4}$ $3.0 \times 10^{-3}$ $1.2 \times 10^{-2}$
| Experiment | $1$ | $2$ | $3$ |
|---|---|---|---|
| $[HI] \ (mol \ L^{-1})$ | $0.005$ | $0.01$ | $0.02$ |
| Rate $(mol \ L^{-1} \ s^{-1})$ | $7.5 \times 10^{-4}$ | $3.0 \times 10^{-3}$ | $1.2 \times 10^{-2}$ |
- A$1$
- B$2$
- C$3$
- D$4$
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Similar Questions
For the reaction $A + B \xrightarrow{K} C$,identify the incorrect order of reaction indicated against the rate expression.
Easy
View SolutionThe following data is given for the reaction between $A$ and $B$:
$S.NO.$ $[A] \ mol \ L^{-1}$ $[B] \ mol \ L^{-1}$ $Rate \ mol \ L^{-1} \ sec^{-1}$ $I$ $1 \times 10^{-2}$ $2 \times 10^{-2}$ $2 \times 10^{-4}$ $II$ $2 \times 10^{-2}$ $2 \times 10^{-2}$ $4 \times 10^{-4}$ $III$ $2 \times 10^{-2}$ $4 \times 10^{-2}$ $8 \times 10^{-4}$
Which of the following are correct statements?
$(a)$ Rate constant of the reaction is $1 \ mol^{-1} \ L \ sec^{-1}$.
$(b)$ Rate law of the reaction is $k[A][B]$.
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactants.
| $S.NO.$ | $[A] \ mol \ L^{-1}$ | $[B] \ mol \ L^{-1}$ | $Rate \ mol \ L^{-1} \ sec^{-1}$ |
| $I$ | $1 \times 10^{-2}$ | $2 \times 10^{-2}$ | $2 \times 10^{-4}$ |
| $II$ | $2 \times 10^{-2}$ | $2 \times 10^{-2}$ | $4 \times 10^{-4}$ |
| $III$ | $2 \times 10^{-2}$ | $4 \times 10^{-2}$ | $8 \times 10^{-4}$ |
Which of the following are correct statements?
$(a)$ Rate constant of the reaction is $1 \ mol^{-1} \ L \ sec^{-1}$.
$(b)$ Rate law of the reaction is $k[A][B]$.
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactants.
Difficult
View SolutionThe rate constant for the reaction, $2 \,N_2O_{5(g)} \rightarrow 2 \,N_2O_{4(g)} + O_{2(g)}$ is $4.98 \times 10^{-4} \,s^{-1}$. What is the order of the reaction?
For a second-order reaction,the rate constant is $8 \times 10^{-5} \, M^{-1} \, \text{min}^{-1}$. In how much time will a $1 \, M$ solution decrease to $0.5 \, M$?
Medium
View Solution........ of a reaction cannot be determined experimentally.
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