The reaction $2 A + B + C \longrightarrow D + E$ is found to be first order in $A$,second order in $B$,and zero order in $C$. What is the effect of increasing the concentration of all reactants twice?
- ARate of reaction increases $8$ times.
- BRate of reaction increases $24$ times.
- CRate of reaction increases $36$ times.
- DRate of reaction remains unaffected.
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Similar Questions
The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.
For the reaction $2HI \rightleftharpoons H_2 + I_2$,the rate of the reaction is proportional to $[HI]^2$. This means that the reaction is
Easy
View SolutionFor conversion of compound $A \rightarrow B$,the rate constant of the reaction was found to be $4.6 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$. The order of the reaction is $..........$
Consider the kinetic data given in the following table for the reaction $A + B + C \rightarrow$ Product.
Experiment No.
$[A] \ (mol \ dm^{-3})$
$[B] \ (mol \ dm^{-3})$
$[C] \ (mol \ dm^{-3})$
Rate of reaction $(mol \ dm^{-3} \ s^{-1})$
$1$
$0.2$
$0.1$
$0.1$
$6.0 \times 10^{-5}$
$2$
$0.2$
$0.2$
$0.1$
$6.0 \times 10^{-5}$
$3$
$0.2$
$0.1$
$0.2$
$1.2 \times 10^{-4}$
$4$
$0.3$
$0.1$
$0.1$
$9.0 \times 10^{-5}$
The rate of the reaction for $[A]=0.15 \ mol \ dm^{-3}, [B]=0.25 \ mol \ dm^{-3}$ and $[C]=0.15 \ mol \ dm^{-3}$ is found to be $Y \times 10^{-5} \ mol \ dm^{-3} \ s^{-1}$. The value of $Y$ is . . . . . .
| Experiment No. | $[A] \ (mol \ dm^{-3})$ | $[B] \ (mol \ dm^{-3})$ | $[C] \ (mol \ dm^{-3})$ | Rate of reaction $(mol \ dm^{-3} \ s^{-1})$ |
| $1$ | $0.2$ | $0.1$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $2$ | $0.2$ | $0.2$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $3$ | $0.2$ | $0.1$ | $0.2$ | $1.2 \times 10^{-4}$ |
| $4$ | $0.3$ | $0.1$ | $0.1$ | $9.0 \times 10^{-5}$ |
The rate of the reaction for $[A]=0.15 \ mol \ dm^{-3}, [B]=0.25 \ mol \ dm^{-3}$ and $[C]=0.15 \ mol \ dm^{-3}$ is found to be $Y \times 10^{-5} \ mol \ dm^{-3} \ s^{-1}$. The value of $Y$ is . . . . . .
MediumIIT 2019
View SolutionThe reaction $2X + Y \to X_2Y$ follows the mechanism given below:
$2X \rightleftharpoons X_2$ (Fast)
$X_2 + Y \to X_2Y$ (Slow)
Determine the order of the reaction.
$2X \rightleftharpoons X_2$ (Fast)
$X_2 + Y \to X_2Y$ (Slow)
Determine the order of the reaction.
Medium
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