For the reaction $2A + B \rightarrow C$,the rate law is given by: $\text{Rate} = k[A][B]$. Which of the following statements is correct regarding this reaction?
- AThe rate of formation of $C$ is twice the rate of disappearance of $A$.
- BThe half-life remains constant.
- CThe unit of $k$ will be $s^{-1}$.
- DThe value of $k$ is independent of the initial concentrations of $A$ and $B$.
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Similar Questions
For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained:
$[AB] \ (mol \ dm^{-3})$ Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$ $0.20$ $2.75 \times 10^{-8}$ $0.40$ $11.0 \times 10^{-8}$ $0.60$ $24.75 \times 10^{-8}$
The order for the decomposition of $AB$ is:
| $[AB] \ (mol \ dm^{-3})$ | Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$ |
| $0.20$ | $2.75 \times 10^{-8}$ |
| $0.40$ | $11.0 \times 10^{-8}$ |
| $0.60$ | $24.75 \times 10^{-8}$ |
The order for the decomposition of $AB$ is:
DifficultKCET 2009
View SolutionExplain the order of reaction for complex reactions by giving examples.
Difficult
View SolutionConsider 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 SolutionWhich of the following statements is $NOT$ true for a reaction having rate law $r=k[H_2][I_2]$?
The 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?
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