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(C) For a first order reaction,the rate law is given by $r = k[A]$.Given: $r = 2.0 	imes 10^{-5} \ M \ sec^{-1}$ and $[A] = 0.01 \ M$.Substituting th

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$346.5$

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(C) For a first order reaction,the rate law is given by $r = k[A]$.Given: $r = 2.0 	imes 10^{-5} \ M \ sec^{-1}$ and $[A] = 0.01 \ M$.Substituting the values: $2.0 	imes 10^{-5} = k 	imes 0.01$.$k = \frac{2.0 	imes 10^{-5}}{10^{-2}} = 2.0 	imes 10^{-3} \ sec^{-1}$.The half-life period $t_{1/2}$ for a first order reaction is $t_{1/2} = \frac{0.693}{k}$.$t_{1/2} = \frac{0.693}{2.0 	imes 10^{-3}} = 0.3465 	imes 10^3 = 346.5 \ sec$.

For a first order reaction $A \to B$,the reaction rate at reactant concentration of $0.01 \ M$ is found to be $2.0 \times 10^{-5} \ M \ sec^{-1}$. The half-life period of the reaction is .......... $sec$.

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