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Question

(C) For a zero-order reaction,the integrated rate equation is given as:$k = \frac{[R_0] - [R]}{t}$where $k$ is the rate constant,$[R_0]$ is the initia

Vedclass · Accepted Answer

$k = \frac{[R_0] - \frac{1}{2}[R_0]}{t_{1/2}}$

Vedclass · Answer

(C) For a zero-order reaction,the integrated rate equation is given as:$k = \frac{[R_0] - [R]}{t}$where $k$ is the rate constant,$[R_0]$ is the initial concentration,and $[R]$ is the concentration at time $t$.At half-life time,$t = t_{1/2}$,the concentration of the reactant is $[R] = \frac{[R_0]}{2}$.Substituting these values into the rate equation:$k = \frac{[R_0] - \frac{[R_0]}{2}}{t_{1/2}}$Thus,the correct expression is $k = \frac{[R_0] - \frac{1}{2}[R_0]}{t_{1/2}}$.Hence,option $(C)$ is the correct answer.

For a zero-order reaction,the correct expression for rate constant $(k)$ at half-life time $(t_{1/2})$ is ($[R_0] =$ initial concentration of reactant).

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