Rate constant 'k' of a reaction varies with temperature 'T' according to the equation:
` log K = log A -E_a =(E_a)/(2.303 R) ((1)/(T))`
where `E_a` is the activation energy. When a graph is plotted for log `,k vs (1)/(T )` a straight line with a slope of - 4250 K is obtained. Calculate ‘`E_a`' for the reaction. (R= 8.314 `JK^(-1) mol^(-1)`)

Explanation

To calculate the activation energy \( E_a \) for the reaction based on the given information, we can follow these steps:

### Step-by-Step Solution

1. **Understand the given equation**: The relationship between the rate constant \( k \) and temperature \( T \) is given by:
\[ \log k = \log A - \frac{E_a}{2.303 R} \left(\frac{1}{T}\right) \]
...