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(B) For a first-order reaction,the rate of reaction is given by $Rate = k[A]^1$. As the concentration of the reactant $[A]$ decreases over time,the ra

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For a first-order reaction,the rate of reaction remains constant.

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(B) For a first-order reaction,the rate of reaction is given by $Rate = k[A]^1$. As the concentration of the reactant $[A]$ decreases over time,the rate of the reaction also decreases. Therefore,the statement that the rate remains constant is incorrect. The half-life of a first-order reaction is $t_{1/2} = 0.693/k$,which is independent of the initial concentration. The unit of the rate constant $k$ for a reaction of order $n$ is $(mol 	ext{ } L^{-1})^{1-n} 	ext{ } s^{-1}$. For $n=2$,the unit is $(mol 	ext{ } L^{-1})^{-1} 	ext{ } s^{-1} = mol^{-1} 	ext{ } L 	ext{ } s^{-1}$.

Which of the following statements is incorrect?

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