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(A) For a zero-order reaction,the half-life is given by $t_{1/2} = \frac{[R]_0}{2k}$.Given $[R]_0 = 2 \ M$ and $t_{1/2} = 1 \ h$,we find the rate cons

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$0.25$

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(A) For a zero-order reaction,the half-life is given by $t_{1/2} = \frac{[R]_0}{2k}$.Given $[R]_0 = 2 \ M$ and $t_{1/2} = 1 \ h$,we find the rate constant $k = \frac{[R]_0}{2t_{1/2}} = \frac{2}{2 	imes 1} = 1 \ M \ h^{-1}$.The time $t$ required for the concentration to change from $[R]_1 = 0.5 \ M$ to $[R]_2 = 0.25 \ M$ is given by $t = \frac{[R]_1 - [R]_2}{k}$.Substituting the values,$t = \frac{0.5 - 0.25}{1} = 0.25 \ h$.

For a reaction $A \rightarrow$ products,the half-life period is $1 \ h$. The initial concentration of reactant $A$ is $2 \ M$. If this reaction is of zero order,how many hours will it take for the concentration of the reactant to decrease from $0.5 \ M$ to $0.25 \ M$?

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