Which one of the following graphs is not appl | vedclass

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(A) For a $1^{st}$ order reaction, the integrated rate equation is $[R] = [R]_0 e^{-kt}$.$(1)$ The plot of $[R]$ vs $t$ is an exponential decay curve,

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(A) For a $1^{st}$ order reaction, the integrated rate equation is $[R] = [R]_0 e^{-kt}$.$(1)$ The plot of $[R]$ vs $t$ is an exponential decay curve, not a straight line.$(2)$ The plot of $\ln[R]$ vs $t$ is a straight line with slope $-k$ and intercept $\ln[R]_0$.$(3)$ The plot of $\log_{10}[R]$ vs $t$ is a straight line with slope $-\frac{k}{2.303}$ and intercept $\log_{10}[R]_0$.$(4)$ The plot of $\log_{10}\frac{[R]_0}{[R]}$ vs $t$ is a straight line with slope $\frac{k}{2.303}$ passing through the origin.Since the graph in option $A$ is shown as a horizontal straight line (which represents a zero-order reaction), it is not applicable for a $1^{st}$ order reaction.

Which one of the following graphs is not applicable for a $1^{st}$ order reaction $(R \rightarrow P)$?

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