Calculate the rate constant of a first order reaction if the half-life of the reaction is $40 \ minute$.
- A$1.733 \times 10^{-2} \ minute^{-1}$
- B$1.951 \times 10^{-2} \ minute^{-1}$
- C$1.423 \times 10^{-2} \ minute^{-1}$
- D$1.256 \times 10^{-2} \ minute^{-1}$
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What is the rate constant of a first-order reaction if the time required to decrease the concentration of the reactant from $1.6 \ M$ to $0.4 \ M$ is $12 \ hours$?
The first order integrated rate equation is
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View SolutionCalculate the rate constant of the first order reaction if $20 \%$ of the reactant decomposes in $15 \ minutes$.
The decomposition of substance $A$ follows first-order kinetics. Flask $I$ contains $1 \ L$ of $1 \ M$ solution of $A$,and flask $II$ contains $100 \ mL$ of $0.6 \ M$ solution of $A$. After $8 \ hours$,the concentration of $A$ in flask $I$ becomes $0.25 \ M$. How many hours will it take for the concentration of $A$ in flask $II$ to become $0.3 \ M$?
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View SolutionIdentify True $(T)$ and False $(F)$ statements of the following for a first-order reaction $R \rightarrow P$.
Statement $I$: $k = \frac{1}{(t_1 - t_2)} \ln \frac{[R]_1}{[R]_2}$
Statement $II$: $k = -\frac{1}{(t_1 - t_2)} \ln \frac{[R]_2}{[R]_1}$
Statement $I$: $k = \frac{1}{(t_1 - t_2)} \ln \frac{[R]_1}{[R]_2}$
Statement $II$: $k = -\frac{1}{(t_1 - t_2)} \ln \frac{[R]_2}{[R]_1}$
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