For a reaction,$A \rightarrow B$,the rate equation is $r = K[A]^0$. If the initial concentration of the reactant is $a \ mol \ dm^{-3}$,find the half-life time of the reaction.
- A$\frac{a}{4k}$
- B$\frac{a}{k}$
- C$\frac{5a}{2k}$
- D$\frac{a}{2k}$
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View SolutionWhich of the following is correct with respect to the graph given?
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$
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