In a reaction,reactant $A$ decomposes $10 \%$ in $1 \ hour$,$20 \%$ in $2 \ hours$ and $30 \%$ in $3 \ hours$. The unit of rate constant of this reaction is
- A$sec^{-1}$
- B$mol \ L^{-1} \ sec^{-1}$
- C$L \ mol^{-1} \ sec^{-1}$
- D$L^{2} \ mol^{-2} \ sec^{-1}$
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The reaction $2A \rightarrow B + C$ follows zero-order kinetics when:
Easy
View SolutionFor a zero order reaction:
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View SolutionWhich among the following is an example of a zero order reaction?
$A$ zero order reaction has a half-life time of $0.2 \ min$. If the initial concentration of the reactant is $0.2 \ mol \ dm^{-3}$,find the rate constant.
Consider the data given below for the hypothetical reaction $A \to X$:
$Time \ (s)$ $Rate \ (mol \ L^{-1} s^{-1})$ $0$ $1.60 \times 10^{-2}$ $10$ $1.60 \times 10^{-2}$ $20$ $1.60 \times 10^{-2}$ $30$ $1.60 \times 10^{-2}$
From the above data,the order of the reaction is:
| $Time \ (s)$ | $Rate \ (mol \ L^{-1} s^{-1})$ |
|---|---|
| $0$ | $1.60 \times 10^{-2}$ |
| $10$ | $1.60 \times 10^{-2}$ |
| $20$ | $1.60 \times 10^{-2}$ |
| $30$ | $1.60 \times 10^{-2}$ |
From the above data,the order of the reaction is:
Medium
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