Medium
For the reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:
- A$1.732 \ mol \ L^{-1}$
- B$3 \ mol \ L^{-1}$
- C$1.02 \times 10^{-4} \ mol \ L^{-1}$
- D$3.4 \times 10^{5} \ mol \ L^{-1}$
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For the non-stoichiometric reaction $2A + B \rightarrow C + D,$ the following kinetic data were obtained in three separate experiments,all at $298 \, K.$
Initial Concentration $(A)$ Initial Concentration $(B)$ Initial rate of formation of $C$ $(mol \, L^{-1} \, s^{-1})$ $0.1 \, M$ $0.1 \, M$ $1.2 \times 10^{-3}$ $0.1 \, M$ $0.2 \, M$ $1.2 \times 10^{-3}$ $0.2 \, M$ $0.1 \, M$ $2.4 \times 10^{-3}$
The rate law for the formation of $C$ is:
| Initial Concentration $(A)$ | Initial Concentration $(B)$ | Initial rate of formation of $C$ $(mol \, L^{-1} \, s^{-1})$ |
| $0.1 \, M$ | $0.1 \, M$ | $1.2 \times 10^{-3}$ |
| $0.1 \, M$ | $0.2 \, M$ | $1.2 \times 10^{-3}$ |
| $0.2 \, M$ | $0.1 \, M$ | $2.4 \times 10^{-3}$ |
The rate law for the formation of $C$ is:
DifficultJEE MAIN 2014
View SolutionWhich of the following statements about the rate constant is $NOT$ true?
Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be
The rate law for the reaction $A^{+} + B^{+} + C \longrightarrow \text{Product}$ is expressed as $\text{Rate} = k[A]^{2}[B]^{1}[C]^{0}$. What is the overall order of the reaction?
$A$ reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is $(i)$ doubled $(ii)$ reduced to half?
Medium
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