For a first-order reaction,if the value of $a/(a - x)$ is $8$ after $10 \text{ minutes}$,what will be the rate constant $K$?
- A$\frac{2.303 \times 3 \log 2}{10}$
- B$\frac{2.303 \times 2 \log 3}{10}$
- C$10^1 \times 2.303 \times 2 \log 3$
- D$10^1 \times 2.303 \times 3 \log 2$
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Similar Questions
What is the rate constant of a first-order reaction if $60 \%$ of the reactant decomposes in $45 \ minutes$?
What is the half-life of a first order reaction if the time required to decrease the concentration of the reactant from $1.0 \ M$ to $0.25 \ M$ is $10 \ hours$ (in $hours$)?
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 a first order reaction,the initial concentration of a reactant is $0.05 \ M$. After $45 \ minutes$,it is decreased by $0.015 \ M$. Calculate the half-life period $(t_{1/2})$ (in $min$)?
If the half-life period of a first order reaction is $138.6 \ minutes$,then the value of the decay constant for the reaction will be:
Medium
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