Which of the following plots is correct for a | vedclass

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(A) For a zero-order reaction,the rate law is given by: $dx/dt = k[A]^0 = k$.This means the rate of reaction is independent of the concentration of th

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(A) For a zero-order reaction,the rate law is given by: $dx/dt = k[A]^0 = k$.This means the rate of reaction is independent of the concentration of the reactant.Therefore,the plot of $dx/dt$ versus $(a-x)$ should be a horizontal line parallel to the $(a-x)$ axis.However,looking at the standard integrated rate equation for a zero-order reaction: $[A] = [A]_0 - kt$,where $[A] = (a-x)$ and $[A]_0 = a$.This gives $(a-x) = a - kt$,or $(a-x) = -kt + a$.Comparing this with the equation of a straight line $y = mx + c$,a plot of $(a-x)$ versus $t$ is a straight line with a negative slope $(-k)$ and an intercept $(a)$.Among the given options,the plot of $(a-x)$ versus $t$ (which is represented by option $A$ where $a$ is the initial concentration and the y-axis represents the concentration at time $t$) is the correct representation for a zero-order reaction.

Which of the following plots is correct for a zero-order reaction?

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