Describe the nature of the following graphs for a zero-order reaction:
$(i)$ Concentration of reactant $\to$ Time
$(ii)$ Concentration of product $\to$ Time
$(i)$ Concentration of reactant $\to$ Time
$(ii)$ Concentration of product $\to$ Time
(N/A) For a zero-order reaction,the rate of reaction is independent of the concentration of the reactant.
$(i)$ The graph of $[R]$ versus $t$ is a straight line with a negative slope equal to $-k$ and an intercept equal to $[R]_0$. The equation is $[R] = -kt + [R]_0$.
$(ii)$ The graph of $[P]$ versus $t$ is a straight line with a positive slope equal to $k$ and an intercept equal to $[P]_0$. The equation is $[P] = kt + [P]_0$.
$(i)$ The graph of $[R]$ versus $t$ is a straight line with a negative slope equal to $-k$ and an intercept equal to $[R]_0$. The equation is $[R] = -kt + [R]_0$.
$(ii)$ The graph of $[P]$ versus $t$ is a straight line with a positive slope equal to $k$ and an intercept equal to $[P]_0$. The equation is $[P] = kt + [P]_0$.
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