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(D) For a first-order reaction,the integrated rate equation is given by: $\log(a - x) = -\frac{kt}{2.303} + \log a$. This equation is of the form $y =

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Both $A$ and $C$.

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(D) For a first-order reaction,the integrated rate equation is given by: $\log(a - x) = -\frac{kt}{2.303} + \log a$. This equation is of the form $y = mx + c$,where the slope $m = -\frac{k}{2.303}$. Thus,a plot of $\log(a - x)$ versus $t$ is a straight line with a negative slope. This matches graph $A$. Additionally,for a first-order reaction,the half-life period is given by: $t_{1/2} = \frac{0.693}{k}$. This shows that $t_{1/2}$ is independent of the initial concentration $a$. Thus,a plot of $t_{1/2}$ versus $a$ is a horizontal line parallel to the $a$-axis. This matches graph $C$. Therefore,both graphs $A$ and $C$ represent a first-order reaction.

$t \ (sec)$	$P \ (mm \ of \ Hg)$
$0$	$35.0$
$360$	$54.0$
$720$	$63.0$

Which of the following graphs represents a first-order reaction?

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$t \ (sec)$ $P \ (mm \ of \ Hg)$

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$360$ $54.0$

$720$ $63.0$

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