(C) For a first-order reaction,the rate law is given by $Rate = k[N_2O_5]^1$.Since the reaction is first-order,the half-life period $(t_{1/2})$ is ind

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(C) For a first-order reaction,the rate law is given by $Rate = k[N_2O_5]^1$.Since the reaction is first-order,the half-life period $(t_{1/2})$ is independent of the initial concentration $(a)$ of the reactant.The formula for half-life is $t_{1/2} = \frac{0.693}{k}$.Therefore,$t_{1/2} \propto a^0$,which means $t_{1/2}$ is constant regardless of the initial concentration $a$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

For the decomposition reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$,the reaction follows first-order kinetics. Which of the following is true?

A
The reaction is bimolecular.
B
$t_{1/2} \propto a$
C
$t_{1/2} \propto a^0$
D
None of these

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Chemical Kinetics

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First Order reaction

$T_{50}$ of a first-order reaction is $10 \ min$. Starting with $10 \ mol \ L^{-1}$,the rate after $20 \ min$ is:

MediumAIIMS 2008

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What is the value of the rate constant for a first-order reaction,if it takes $15 \ min$ for the consumption of $20 \%$ of the reactants?

EasyMHT CET 2020

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The rate constant of a first-order reaction is $10^{-3} \ min^{-1}$ and the initial concentration of the reactant is $0.2 \ mol \ dm^{-3}$. What percentage of the reactant will be converted into product in $200 \ min$?

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The half-life of a first-order reaction is $900 \text{ s}$. If the initial concentration of the reactant is $0.08 \text{ mol dm}^{-3}$, find the concentration that remains after $35 \text{ minutes}$?

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Identify $True$ $(T)$ and $False$ $(F)$ statements for the following equations related to a first-order reaction $R \rightarrow P$:
$(i) \ln [R] = -kt + \ln [R]_{0}$
$(ii) \ln [R] = +kt + \ln [R]_{0}$

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For the decomposition reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$,the reaction follows first-order kinetics. Which of the following is true?

Similar Questions

$T_{50}$ of a first-order reaction is $10 \ min$. Starting with $10 \ mol \ L^{-1}$,the rate after $20 \ min$ is:

What is the value of the rate constant for a first-order reaction,if it takes $15 \ min$ for the consumption of $20 \%$ of the reactants?

The rate constant of a first-order reaction is $10^{-3} \ min^{-1}$ and the initial concentration of the reactant is $0.2 \ mol \ dm^{-3}$. What percentage of the reactant will be converted into product in $200 \ min$?

The half-life of a first-order reaction is $900 \text{ s}$. If the initial concentration of the reactant is $0.08 \text{ mol dm}^{-3}$, find the concentration that remains after $35 \text{ minutes}$?

Identify $True$ $(T)$ and $False$ $(F)$ statements for the following equations related to a first-order reaction $R \rightarrow P$:$(i) \ln [R] = -kt + \ln [R]_{0}$$(ii) \ln [R] = +kt + \ln [R]_{0}$

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Identify $True$ $(T)$ and $False$ $(F)$ statements for the following equations related to a first-order reaction $R \rightarrow P$:
$(i) \ln [R] = -kt + \ln [R]_{0}$
$(ii) \ln [R] = +kt + \ln [R]_{0}$