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(A) The time required to reduce the concentration of the reactant to half of its initial value is known as the half-life $(t_{1/2})$.For a zero-order

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increases two-fold

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(A) The time required to reduce the concentration of the reactant to half of its initial value is known as the half-life $(t_{1/2})$.For a zero-order reaction,the half-life is given by the formula:$t_{1/2} = \frac{[A]_0}{2k}$where $[A]_0$ is the initial concentration and $k$ is the rate constant.If the initial concentration is doubled,i.e.,$[A]_0' = 2[A]_0$,then the new half-life becomes:$t_{1/2}' = \frac{2[A]_0}{2k} = 2 	imes t_{1/2}$Therefore,the time required for half the reactant to be consumed increases two-fold.

$[R] \ (M)$	$1.0$	$0.76$	$0.40$	$0.10$
$t \ (min)$	$0.0$	$0.05$	$0.12$	$0.18$

In a zero-order reaction,if the initial concentration of the reactant is doubled,the time required for half the reactant to be consumed:

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The half-life period for a certain zero-order reaction is $10 \text{ min}$. How much time is required for this reaction to complete $100\%$ (in $\text{ min}$)?

For the reaction $R \rightarrow P$,the concentration of $R$ is measured as a function of time and the following data is obtained:

$[R] \ (M)$ $1.0$ $0.76$ $0.40$ $0.10$

$t \ (min)$ $0.0$ $0.05$ $0.12$ $0.18$

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