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Examine the graph and linear regression shown below and choose the answer that is FALSE. 1.2 y = -0.0034x +0.9996 R2 = 1 0.8

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\bf \text{ This graph represents }Zero\;order\text{ reaction.}\\

\bf \text{Integrated rate law}\\ {\;\;\;\;\;}[A]=-kt+[A]_0\\\\ {\;\;\;\;\;}t_{1/2}=\frac{[A]_0}{2k}\\\\ {\;\;\;\;\;}Unit\;of\;k:M/s

\bf \text{ From the given equation we have }\\\\ {\;\;\;\;\;\;}k=0.0034M/s\\\\ {\;\;\;\;\;\;}[A]_0=1M\\\\ {\;\;\;\;\;\;}t_{1/2}=\frac{1M}{2\times 0.0034M/s}\approx 150\;s

\therefore \textbf{ The FALSE statement is :}\\\\ \textbf{\;\;\;\;\;\;\;\;\;The reaction has a half-life that does not depend on the initial concentration}\\ \textbf{\;\;\;\;\;\;\;\; of the reactant. }

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