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
For the reaction $A + 2B \rightleftharpoons 2C + D$,if the concentration of $A$ is increased four times and the concentration of $B$ is reduced to half,the rate of the reaction will be:
Easy
View SolutionWhich of the following statements is true regarding the order of a reaction?
Medium
View SolutionThe experimental data for the reaction $2A + B_2 \to 2AB$ is given below. Determine the rate equation for the reaction.
$Exp.$ $[A]_0$ $[B_2]_0$ $Rate \ (mol \ L^{-1} \ s^{-1})$ $(1)$ $0.50$ $0.50$ $1.6 \times 10^{-4}$ $(2)$ $0.50$ $1.00$ $3.2 \times 10^{-4}$ $(3)$ $1.00$ $1.00$ $3.2 \times 10^{-4}$
| $Exp.$ | $[A]_0$ | $[B_2]_0$ | $Rate \ (mol \ L^{-1} \ s^{-1})$ |
| $(1)$ | $0.50$ | $0.50$ | $1.6 \times 10^{-4}$ |
| $(2)$ | $0.50$ | $1.00$ | $3.2 \times 10^{-4}$ |
| $(3)$ | $1.00$ | $1.00$ | $3.2 \times 10^{-4}$ |
MediumAIPMT 1997
View SolutionWhat is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
Difficult
View SolutionFor the reaction $AB_5 \to AB + 4B$,if $- \frac{d[AB_5]}{dt} = K_1[AB_5]$ and $\frac{d[B]}{dt} = K_2[AB_5]$,then:
Medium
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