Q.The rate constant of a first-order reaction is $3.0 \times 10^{-6} \text{ s}^{-1}$ . If the initial concentration of the reactant is $0.10 \text{ mol L}^{-1}$ , the rate of reaction is:

3.0 \times 10^{-7} \text{ mol L}^{-1} \text{ s}^{-1}

3.0 \times 10^{-6} \text{ mol L}^{-1} \text{ s}^{-1}

3.0 \times 10^{-5} \text{ mol L}^{-1} \text{ s}^{-1}

3.0 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}

The correct solution involves applying the fundamental concept to derive the final value step by step...

Already a member? Login here

Q.The rate constant of a first-order reaction is 3.0×10−6 s−13.0 \times 10^{-6} \text{ s}^{-1}3.0×10−6 s−1. If the initial concentration of the reactant is 0.10 mol L−10.10 \text{ mol L}^{-1}0.10 mol L−1, the rate of reaction is: