Calculate the rate constant of the first order reaction if $80 \%$ of the reactant decomposes in $60 \ minutes$.
- A$2.68 \times 10^{-2} \ minute^{-1}$
- B$5.36 \times 10^{-2} \ minute^{-1}$
- C$1.34 \times 10^{-2} \ minute^{-1}$
- D$8.1 \times 10^{-2} \ minute^{-1}$
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Similar Questions
Following data was obtained for the first order decomposition of $SO_2Cl_{2(g)}$ at constant volume:
$SO_2Cl_{2(g)} \to SO_{2(g)} + Cl_{2(g)}$
$S. No.$ $Time$ $(s)$ $Total$ $pressure$ $(atm)$ $1$ $0$ $0.5$ $2$ $100$ $0.6$
Calculate the rate constant.
$SO_2Cl_{2(g)} \to SO_{2(g)} + Cl_{2(g)}$
| $S. No.$ | $Time$ $(s)$ | $Total$ $pressure$ $(atm)$ |
| $1$ | $0$ | $0.5$ |
| $2$ | $100$ | $0.6$ |
Calculate the rate constant.
Medium
View SolutionFor the $1^{st}$ order reaction,the half-life is $5 \ minutes$ when $[A] = 0.1 \ M$. If the concentration of $[A]$ becomes twice,then the half-life becomes:
Easy
View SolutionWhat 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 rate constant of a reaction is $0.693 \times 10^{-2} \ min^{-1}$. What is the half-life period (in $s$)?
In a first order reaction $A \to B,$ if $k$ is the rate constant and the initial concentration of the reactant $A$ is $0.5 \ M,$ then the half-life is:
Medium
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