Mention True $(T)$ and False $(F)$ statement of the following for reaction $R \to P$.
Rate $= -\frac{d[R]}{dt} = k[R]^0$
Rate $= -\frac{d[R]}{dt} = k$

(A) For a zero-order reaction $R \to P$,the rate law is given by: $\text{Rate} = k[R]^0$.
Since any non-zero value raised to the power of $0$ is $1$,we have $[R]^0 = 1$.
Therefore,the rate expression simplifies to: $\text{Rate} = k$.
Both statements are mathematically equivalent and represent the definition of a zero-order reaction.
Thus,both statements are True $(T)$.