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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What is the unit of rate constant for the zero order reaction?
Mention True $(T)$ and False $(F)$ statements for the following expressions related to a zero-order reaction $R \to P$:
$I. \ k = \frac{[R]_0}{2 t_{1/2}}$
$II. \ t_{1/2} = \frac{[R]_0}{4k}$
$I. \ k = \frac{[R]_0}{2 t_{1/2}}$
$II. \ t_{1/2} = \frac{[R]_0}{4k}$
Easy
View SolutionFor a zero order reaction:
Easy
View SolutionFor a zero-order reaction,the correct expression for rate constant $(k)$ at half-life time $(t_{1/2})$ is ($[R_0] =$ initial concentration of reactant).
The rate constant of the reaction $A \rightarrow B$ is $0.6 \times 10^{-3} \, mol \, L^{-1} \, s^{-1}.$ If the concentration of $A$ is $5 \, M,$ then the concentration of $B$ after $20$ minutes is ......... $M.$
MediumNEET 2015
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