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(D) $1$. The unit of the rate constant is $	ext{mol L}^{-1} 	ext{ s}^{-1}$, which is the characteristic unit for a zero-order reaction.$2$. For a ze

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None of the above

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(D) $1$. The unit of the rate constant is $	ext{mol L}^{-1} 	ext{ s}^{-1}$, which is the characteristic unit for a zero-order reaction.$2$. For a zero-order reaction, the rate is given by $	ext{Rate} = k[X]^0 = k$. Thus, the rate is independent of the concentration of the reactant $X$.$3$. Statement $A$ is false because the rate remains constant regardless of the concentration of $X$.$4$. Statement $B$ is false because the reaction is zero-order, not second-order.$5$. Statement $C$ is false because for a zero-order reaction, the half-life $t_{1/2} = \frac{[R]_0}{2k}$, which depends on the initial concentration.$6$. Statement $D$ is false because the decomposition of $N_2O_5$ is a first-order reaction.$7$. Statement $E$ is false because the plot of $\ln \frac{[R]_0}{[R]}$ vs time is linear only for first-order reactions. For zero-order, $[R]$ vs time is linear.$8$. Since none of the statements $A, B, C, D,$ or $E$ are true, the correct choice is 'None of the above'.

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