The rate constant for a zero order reaction i | vedclass

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(D) For a zero order reaction,the integrated rate equation is given by: $[A] = [A]_0 - kt$. Here,$[A]$ is the final concentration,$[A]_0$ is the initi

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$1.0$

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(D) For a zero order reaction,the integrated rate equation is given by: $[A] = [A]_0 - kt$. Here,$[A]$ is the final concentration,$[A]_0$ is the initial concentration,$k$ is the rate constant,and $t$ is the time. Given: $k = 2 	imes 10^{-2} \ mol \ L^{-1} s^{-1}$,$t = 25 \ s$,and $[A] = 0.5 \ M$. Substituting the values into the equation: $0.5 = [A]_0 - (2 	imes 10^{-2} 	imes 25)$. $0.5 = [A]_0 - 0.5$. $[A]_0 = 0.5 + 0.5 = 1.0 \ M$.

The rate constant for a zero order reaction is $2 \times 10^{-2} \ mol \ L^{-1} s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,the initial concentration must have been $:-$ (in $M$)

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