In the following reaction A rightarrow B + C, | vedclass

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(C) The unit of the rate constant $k$ is $M \cdot s^{-1}$,which indicates a zero-order reaction.For a zero-order reaction: $[A]_t = [A]_0 - kt$.Given:

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$0.4 \ M, 0.6 \ M$

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(C) The unit of the rate constant $k$ is $M \cdot s^{-1}$,which indicates a zero-order reaction.For a zero-order reaction: $[A]_t = [A]_0 - kt$.Given: $[A]_0 = 1 \ M$,$k = 0.001 \ M \cdot s^{-1}$,and $t = 10 \ minutes = 600 \ s$.$[A]_t = 1 - (0.001 	imes 600) = 1 - 0.6 = 0.4 \ M$.The concentration of $B$ formed is $[B]_t = [A]_0 - [A]_t = 1 - 0.4 = 0.6 \ M$.Therefore,$[A] = 0.4 \ M$ and $[B] = 0.6 \ M$.

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

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