The rate law equation for a reaction is $R = k[x][y]$. The rate of reaction doubles when:
- Aconcentration of $x$ is kept constant and concentration of $y$ is halved
- Bconcentration of both $x$ and $y$ is doubled
- Cconcentration of $x$ is doubled and concentration of $y$ is kept constant
- Dconcentration of $y$ is doubled and concentration of $x$ is halved
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Similar Questions
The following graph shows how $T_{1/2}$ (half-life) of a reactant $R$ changes with the initial reactant concentration $a_0$. The order of the reaction will be:
What is the time taken for the $3^{rd}$ half-life of a second-order decomposition reaction,given that its first half-life is $20 \ s$ (in $s$)?
Medium
View SolutionThe 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
View SolutionFor 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.
Difficult
View SolutionGive the relation between half-life $(t_{1/2})$ and initial concentration of reactant $([R]_0)$ for an $(n-1)^{th}$ order reaction.
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