(B) The rate law for the decomposition of $N_2O_5$ is given by $Rate = k[N_2O_5]$.Given:$Rate = 1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$$k = 3.4 \

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(B) The rate law for the decomposition of $N_2O_5$ is given by $Rate = k[N_2O_5]$.Given:$Rate = 1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$$k = 3.4 \times 10^{-5} \ s^{-1}$Substituting the values in the rate equation:$1.02 \times 10^{-4} = (3.4 \times 10^{-5}) \times [N_2O_5]$$[N_2O_5] = \frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}}$$[N_2O_5] = 3 \ mol \ L^{-1}$Therefore,the correct option is $B$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

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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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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For a certain reaction $A \to P$,the half-life for different initial concentrations of $A$ is mentioned below:
$[A_0]$ $0.1 \ M$ $0.025 \ M$
$t_{1/2} \ (s)$ $100 \ s$ $50 \ s$

Which of the following option$(s)$ is/are correct?

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The temperature coefficient of most reactions lies between $.......$.

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The mechanism of the reaction $2NO_{(g)} + Br_{2(g)} \rightarrow 2NOBr_{(g)}$ is given by:
$1) NO_{(g)} + Br_{2(g)} \rightleftharpoons NOBr_{2(g)}$ (fast)
$2) NOBr_{2(g)} + NO_{(g)} \rightarrow 2NOBr_{(g)}$ (slow)
If the second step is the rate-determining step,what is the order of the reaction with respect to $NO_{(g)}$?

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For a given reaction $t_{1/2} = \frac{1}{Ka}$. The order of the reaction is

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For the reaction $A + B \to \text{products}$,it is found that the rate of the reaction is proportional to the concentration of $A$,but it is independent of the concentration of $B$. Then:

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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:

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For a certain reaction $A \to P$,the half-life for different initial concentrations of $A$ is mentioned below:$[A_0]$$0.1 \ M$$0.025 \ M$$t_{1/2} \ (s)$$100 \ s$$50 \ s$Which of the following option$(s)$ is/are correct?

The temperature coefficient of most reactions lies between $.......$.

For a given reaction $t_{1/2} = \frac{1}{Ka}$. The order of the reaction is

For the reaction $A + B \to \text{products}$,it is found that the rate of the reaction is proportional to the concentration of $A$,but it is independent of the concentration of $B$. Then:

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For a certain reaction $A \to P$,the half-life for different initial concentrations of $A$ is mentioned below:
$[A_0]$ $0.1 \ M$ $0.025 \ M$
$t_{1/2} \ (s)$ $100 \ s$ $50 \ s$

Which of the following option$(s)$ is/are correct?