For a reaction, the activation energy is zero. What is the value of rate constant at `300 K` if `k=1.6 xx 10^(6)s^(-1)` at 280 K
`(R= 8.31 JK^(-1)mol^(-1))`?

Explanation

To solve the problem, we need to determine the rate constant \( K_2 \) at a temperature of 300 K, given that the activation energy is zero and the rate constant \( K_1 \) at 280 K is \( 1.6 \times 10^6 \, s^{-1} \).

### Step-by-Step Solution:

1. **Identify the given values:**
- \( K_1 = 1.6 \times 10^6 \, s^{-1} \) (rate constant at \( T_1 = 280 \, K \))
- \( T_1 = 280 \, K \)
- \( T_2 = 300 \, K \)
...