(B) The given reaction is $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$.Since the unit of the rate constant is $s^{-1}$,it is a first-order r

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(B) The given reaction is $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$.Since the unit of the rate constant is $s^{-1}$,it is a first-order reaction.The rate law expression is given by: $\text{Rate} = k[N_2O_5]$.Substituting the given values: $1.02 \times 10^{-4} = 3.4 \times 10^{-5} \times [N_2O_5]$.Therefore,$[N_2O_5] = \frac{1.02 \times 10^{-4}}{3.4 \times 10^{-5}} = 3.0 \ mol \ L^{-1}$.

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

Medium

For the reaction $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. What is the concentration of $N_2O_5$?

MHT CET 2024 All MHT CET

A
$1.7 \ mol \ L^{-1}$
B
$3.0 \ mol \ L^{-1}$
C
$3.4 \ mol \ L^{-1}$
D
$5.1 \ mol \ L^{-1}$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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Identify the reaction intermediate.

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For the reaction $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. What is the concentration of $N_2O_5$?

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$A$ complex reaction takes place in $2$ steps:$(I)$ $NO_{2(g)} + F_{2(g)} \rightarrow NO_2F_{(g)} + F_{(g)}$ (slow)$(II)$ $F_{(g)} + NO_{2(g)} \rightarrow NO_2F_{(g)}$ (fast)Identify the reaction intermediate.

The inversion of cane sugar is represented by $C_{12}H_{22}O_{11} + H_2O \to C_6H_{12}O_6 + C_6H_{12}O_6$. It is a reaction of

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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$A$ complex reaction takes place in $2$ steps:
$(I)$ $NO_{2(g)} + F_{2(g)} \rightarrow NO_2F_{(g)} + F_{(g)}$ (slow)
$(II)$ $F_{(g)} + NO_{2(g)} \rightarrow NO_2F_{(g)}$ (fast)
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$[A_0]$ $0.1 \ M$ $0.025 \ M$
$t_{1/2} \ (s)$ $100 \ s$ $50 \ s$

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

Calculate the overall order of a reaction which has the rate expression:
$(a)$ $\text{Rate} = k[A]^{1/2}[B]^{3/2}$
$(b)$ $\text{Rate} = k[A]^{3/2}[B]^{-1}$