Difficult
For the reaction $2A + B \to C$,the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is
$[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Initial Rate $(mol \ L^{-1} \ s^{-1})$ $0.05$ $0.05$ $0.045$ $0.10$ $0.05$ $0.090$ $0.20$ $0.10$ $0.72$
| $[A] \ (mol \ L^{-1})$ | $[B] \ (mol \ L^{-1})$ | Initial Rate $(mol \ L^{-1} \ s^{-1})$ |
| $0.05$ | $0.05$ | $0.045$ |
| $0.10$ | $0.05$ | $0.090$ |
| $0.20$ | $0.10$ | $0.72$ |
- ARate $= k[A]^2[B]^2$
- BRate $= k[A][B]^2$
- CRate $= k[A][B]$
- DRate $= k[A]^2[B]$
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Similar Questions
Identify the reaction intermediate of the following reaction sequence:
$(i)$ $2 SO_{2(g)} + 2 NO_{2(g)} \rightarrow 2 SO_{3(g)} + 2 NO_{(g)}$
$(ii)$ $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$
--------------------------------------------------
Overall: $2 SO_{2(g)} + O_{2(g)} \rightarrow 2 SO_{3(g)}$
$(i)$ $2 SO_{2(g)} + 2 NO_{2(g)} \rightarrow 2 SO_{3(g)} + 2 NO_{(g)}$
$(ii)$ $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$
--------------------------------------------------
Overall: $2 SO_{2(g)} + O_{2(g)} \rightarrow 2 SO_{3(g)}$
DifficultMHT CET 2023
View SolutionThe rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:
DifficultAIPMT 2011
View SolutionFor a chemical reaction,$2A + 2B \to C + D$,the order of reaction is $1$ with respect to $A$ and $1$ with respect to $B$. The initial rate of the reaction is $4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. When $50\%$ of the reactants are converted into products,the rate of the reaction would become:
Medium
View SolutionWhich among the following reactions can be an example of a pseudo first order reaction?
The following results are obtained for the reaction $S + Nu \rightarrow \text{product}$. By which reaction mechanism does this reaction occur?
Experiment $[S]$ $[Nu]$ Rate $1$ $0.1$ $0.1$ $2.2 \times 10^{-3}$ $2$ $0.2$ $0.1$ $4.4 \times 10^{-3}$ $3$ $0.1$ $0.2$ $4.4 \times 10^{-3}$
| Experiment | $[S]$ | $[Nu]$ | Rate |
|---|---|---|---|
| $1$ | $0.1$ | $0.1$ | $2.2 \times 10^{-3}$ |
| $2$ | $0.2$ | $0.1$ | $4.4 \times 10^{-3}$ |
| $3$ | $0.1$ | $0.2$ | $4.4 \times 10^{-3}$ |
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