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(B) For a zero order reaction: $Rate = k[Reactant]^0 = k$. Thus,graph $(a)$ (Rate vs Time) is constant,representing zero order. $t_{1/2} = [A]_0 / (2k

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$(a)$ and $(b)$ Zero order; $(c)$ and $(e)$ First order

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(B) For a zero order reaction: $Rate = k[Reactant]^0 = k$. Thus,graph $(a)$ (Rate vs Time) is constant,representing zero order. $t_{1/2} = [A]_0 / (2k)$. Thus,graph $(b)$ ($t_{1/2}$ vs Initial concentration) is a straight line passing through the origin,representing zero order. For a first order reaction: $Rate = k[Concentration]$. Thus,graph $(e)$ (Rate vs Concentration) is a straight line passing through the origin,representing first order. $[A]_t = [A]_0 e^{-kt}$. Thus,graph $(c)$ (Concentration vs Time) is an exponential decay curve,representing first order. Graph $(d)$ shows concentration independent of time,which is not standard for these kinetics. Therefore,$(a)$ and $(b)$ are zero order,while $(c)$ and $(e)$ are first order.

$[A_0]$	$0.1 \ M$	$0.025 \ M$
$t_{1/2} \ (s)$	$100 \ s$	$50 \ s$

For the following graphs,choose the correct option regarding the order of reaction:

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