Which of the following graphs is incorrect fo | vedclass

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(C) For a first-order reaction,the rate law is given by: $	ext{Rate} = k[A]$.This shows that the rate is directly proportional to the concentration o

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(C) For a first-order reaction,the rate law is given by: $	ext{Rate} = k[A]$.This shows that the rate is directly proportional to the concentration of the reactant,so the graph of rate versus concentration is a straight line passing through the origin.The half-life $(t_{1/2})$ for a first-order reaction is given by: $t_{1/2} = \frac{0.693}{k}$.This shows that $t_{1/2}$ is independent of the initial concentration,so the graph of $t_{1/2}$ versus concentration is a horizontal line.The concentration of the reactant at time $t$ is given by: $[A]_t = [A]_0 e^{-kt}$.This shows that the concentration decreases exponentially with time,not linearly.Therefore,the graph of concentration versus time (linear) is incorrect for a first-order reaction.

Which of the following graphs is incorrect for a first-order reaction? $A \rightarrow B$

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