The rate equation for a reaction $A \rightarrow B$ is $r=k[A]^{0}$. If the initial concentration of the reactant is $a \ mol \ dm^{-3}$,the half-life period of the reaction is
- A$\frac{a}{2k}$
- B$\frac{k}{a}$
- C$\frac{a}{k}$
- D$\frac{2a}{k}$
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Similar Questions
Calculate the rate constant of a zero order reaction if it is $90 \%$ completed in $90 \ s$.
Which among the following is an example of a zero order reaction?
Which of the following graphs represents a zero order reaction?
($a = $ initial concentration of reactant,
$x = $ concentration of reactant consumed,
$t = $ time)
($a = $ initial concentration of reactant,
$x = $ concentration of reactant consumed,
$t = $ time)
The concentration of $R$ in the reaction $R \rightarrow P$ was measured as a function of time and the following data is obtained:
$[R] \text{ (molar)}$ $1.0$ $0.75$ $0.40$ $0.10$ $t \text{ (min.)}$ $0.0$ $0.05$ $0.12$ $0.18$
The order of the reaction is:
| $[R] \text{ (molar)}$ | $1.0$ | $0.75$ | $0.40$ | $0.10$ |
| $t \text{ (min.)}$ | $0.0$ | $0.05$ | $0.12$ | $0.18$ |
The order of the reaction is:
MediumIIT 2010
View SolutionThe rate constant of a zero-order reaction is $0.2 \ mol \ m^{-3} \ h^{-1}$. If the concentration of the reactant after $30 \ minutes$ is $0.05 \ mol \ m^{-3}$,then its initial concentration will be ....... $mol \ m^{-3}$.
Medium
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