Consider the following reactant samples:I. 1 | vedclass

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(C) The rate of reaction $r$ for a non-zero order reaction depends on the concentration of reactants. Assuming a simple second-order reaction $r = k[A

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$III$

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(C) The rate of reaction $r$ for a non-zero order reaction depends on the concentration of reactants. Assuming a simple second-order reaction $r = k[A][B]$,we calculate the molar concentrations $(M = mol/L)$:$I$. $[A] = 1 \ mol / 1 \ L = 1 \ M$,$[B] = 2 \ mol / 1 \ L = 2 \ M$. Rate $r_I = k(1)(2) = 2k$.$II$. $[A] = 2 \ mol / 2 \ L = 1 \ M$,$[B] = 2 \ mol / 2 \ L = 1 \ M$. Rate $r_{II} = k(1)(1) = 1k$.$III$. $[A] = 0.2 \ mol / 0.1 \ L = 2 \ M$,$[B] = 0.2 \ mol / 0.1 \ L = 2 \ M$. Rate $r_{III} = k(2)(2) = 4k$.Comparing the rates,$r_{III} > r_I > r_{II}$. Therefore,sample $III$ reacts at the highest rate.

$t \ (s)$	$0$	$30$	$60$	$90$
$[\text{Ester}] \ (mol \ L^{-1})$	$0.55$	$0.31$	$0.17$	$0.085$

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$t \ (s)$ $0$ $30$ $60$ $90$

$[\text{Ester}] \ (mol \ L^{-1})$ $0.55$ $0.31$ $0.17$ $0.085$

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