In the following reaction A to B + C, the rat | vedclass

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(C) The reaction is a zero-order reaction because the unit of the rate constant is $M \ s^{-1}.$The integrated rate equation for a zero-order reaction

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$0.4 \ M, \ 0.6 \ M$

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(C) The reaction is a zero-order reaction because the unit of the rate constant is $M \ s^{-1}.$The integrated rate equation for a zero-order reaction is $[A]_t = [A]_0 - Kt.$Given:$[A]_0 = 1 \ M$$K = 0.001 \ M \ s^{-1}$$t = 10 \ minutes = 10 	imes 60 \ s = 600 \ s$Calculating the concentration of $A$ at time $t$:$[A]_t = 1 - (0.001 	imes 600) = 1 - 0.6 = 0.4 \ M.$Since the stoichiometry of the reaction $A 	o B + C$ is $1:1,$ the concentration of $B$ formed is equal to the amount of $A$ consumed:$[B]_t = [A]_0 - [A]_t = 1 - 0.4 = 0.6 \ M.$Therefore,the concentrations of $A$ and $B$ are $0.4 \ M$ and $0.6 \ M$ respectively.

In the following reaction $A \to B + C,$ the rate constant is $0.001 \ M \ s^{-1}.$ If we start with $1 \ M$ of $A,$ then the concentrations of $A$ and $B$ after $10 \ minutes$ are respectively:

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