Question

The rate constant $\left(k\right)$ of a first order reaction, $A⟶Product$, is $60\times {10}^{-4}{min}^{-1}$. Its rate at $\left[A\right]=0.01$ $mol$ $L^{-1}$ would be:

• A. $60\times {10}^{-6}$ $mol$ $L^{-1}{min}^{-1}$
• B. $36\times {10}^{-4}$ $mol$ $L^{-1}{min}^{-1}$
• C. $60\times {10}^{-2}$ $mol$ $L^{-1}{min}^{-1}$
• D. $36\times {10}^{-1}$ $mol$ $L^{-1}{min}^{-1}$

Answer 1

The correct option is A $60\times {10}^{-6}$ $mol$ $L^{-1}{min}^{-1}$