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(A) For a zero-order reaction,the rate law is given by: $Rate = k[R]^0 = k$.Integrating the rate equation $-\frac{d[R]}{dt} = k$ gives $[R] = -kt + [R

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$(i) T, (ii) F$

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(A) For a zero-order reaction,the rate law is given by: $Rate = k[R]^0 = k$.Integrating the rate equation $-\frac{d[R]}{dt} = k$ gives $[R] = -kt + [R]_0$.Rearranging this equation to solve for the rate constant $k$:$kt = [R]_0 - [R]$$k = \frac{[R]_0 - [R]}{t}$.Comparing this with the given statements:Statement $(i)$ is $k = \frac{[R]_0 - [R]}{t}$,which is correct $(T)$.Statement $(ii)$ is $k = \frac{[R] - [R]_0}{t}$,which is incorrect $(F)$.Therefore,the correct option is $(i) T, (ii) F$.

Mention True $(T)$ and False $(F)$ statements for the following expressions related to a zero-order reaction $R \to P$:
$(i) \ k = \frac{[R]_0 - [R]}{t}$
$(ii) \ k = \frac{[R] - [R]_0}{t}$

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Mention True $(T)$ and False $(F)$ statements for the following expressions related to a zero-order reaction $R \to P$:$(i) \ k = \frac{[R]_0 - [R]}{t}$$(ii) \ k = \frac{[R] - [R]_0}{t}$