Medium
For the reaction $2NO_{(g)} + O_{2_{(g)}} \rightarrow 2NO_{2_{(g)}}$,the volume of the reaction vessel is suddenly reduced to half of its original volume. If the reaction is first order with respect to $O_2$ and second order with respect to $NO$,the rate of the reaction will:
- AIncrease $8$ times its initial value.
- BIncrease $4$ times its initial value.
- CBecome $1/4$ of its initial value.
- DBecome $1/8$ of its initial value.
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Similar Questions
Order of a reaction is decided by
Medium
View Solution$t_{1/2} =$ constant confirms the first order reaction. If $a^2 t_{1/2} =$ constant,it confirms that the order of reaction is ($a =$ initial concentration of reactant).
Medium
View SolutionDuring the kinetic study of the reaction,$2A + B \rightarrow C + D,$ the following results were obtained:
$Run$ $[A] / mol \ L^{-1}$ $[B] / mol \ L^{-1}$ Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$ $I.$ $0.1$ $0.1$ $6.0 \times 10^{-3}$ $II.$ $0.3$ $0.2$ $7.2 \times 10^{-2}$ $III.$ $0.3$ $0.4$ $2.88 \times 10^{-1}$ $IV.$ $0.4$ $0.1$ $2.40 \times 10^{-2}$
Based on the above data,which one of the following is correct?
| $Run$ | $[A] / mol \ L^{-1}$ | $[B] / mol \ L^{-1}$ | Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$ |
| $I.$ | $0.1$ | $0.1$ | $6.0 \times 10^{-3}$ |
| $II.$ | $0.3$ | $0.2$ | $7.2 \times 10^{-2}$ |
| $III.$ | $0.3$ | $0.4$ | $2.88 \times 10^{-1}$ |
| $IV.$ | $0.4$ | $0.1$ | $2.40 \times 10^{-2}$ |
Based on the above data,which one of the following is correct?
What is the molecularity and order of the following reaction if the rate law is $\text{rate} = k[O_3][O]$ respectively?
$O_{3(g)} + O_{(g)} \longrightarrow 2O_{2(g)}$
$O_{3(g)} + O_{(g)} \longrightarrow 2O_{2(g)}$
For the reaction $X_{2(g)} + Y_{2(g)} \rightarrow 2XY_{(g)}$,the following data are observed:
$[X_{2}] \ (M)$ $[Y_{2}] \ (M)$ Rate of appearance of $XY \ (M \ sec^{-1})$ $0.1$ $0.1$ $5 \times 10^{-6}$ $0.2$ $0.1$ $10^{-5}$ $0.2$ $0.2$ $4 \times 10^{-5}$
Calculate the rate constant of the reaction (in $M^{1-n} \ sec^{-1}$),where $n$ is the order of the reaction.
| $[X_{2}] \ (M)$ | $[Y_{2}] \ (M)$ | Rate of appearance of $XY \ (M \ sec^{-1})$ |
| $0.1$ | $0.1$ | $5 \times 10^{-6}$ |
| $0.2$ | $0.1$ | $10^{-5}$ |
| $0.2$ | $0.2$ | $4 \times 10^{-5}$ |
Calculate the rate constant of the reaction (in $M^{1-n} \ sec^{-1}$),where $n$ is the order of the reaction.
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