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(B) For a zero order reaction,the rate law is given by: $Rate = k[A]^0 = k$. Integrating this with respect to time,we get the integrated rate equation

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linear with $-ve$ slope and non zero $+ve$ intercept

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(B) For a zero order reaction,the rate law is given by: $Rate = k[A]^0 = k$. Integrating this with respect to time,we get the integrated rate equation: $[A] = -kt + [A]_0$. This equation follows the form of a straight line equation $y = mx + c$,where $y = [A]$,$x = t$,$m = -k$ (slope),and $c = [A]_0$ (intercept). Therefore,the plot of concentration $[A]$ versus time $t$ is a straight line with a negative slope equal to $-k$ and a non-zero positive intercept equal to $[A]_0$ on the concentration axis.

For a zero order reaction,the plot of concentration of reactant $vs$ time is (Hint: Consider the intercept on the concentration axis)

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