Q.The activation energy of a reaction is $0$ . If the rate constant at $200 \text{ K}$ is $1.6 \times 10^6 \text{ s}^{-1}$ , the rate constant at $400 \text{ K}$ will be:

3.2 \times 10^6 \text{ s}^{-1}

1.6 \times 10^6 \text{ s}^{-1}

0.8 \times 10^6 \text{ s}^{-1}

6.4 \times 10^6 \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 activation energy of a reaction is 000. If the rate constant at 200 K200 \text{ K}200 K is 1.6×106 s−11.6 \times 10^6 \text{ s}^{-1}1.6×106 s−1, the rate constant at 400 K400 \text{ K}400 K will be: