In general, it is observed that the rate of a chemical reaction doubles with every `10^(@)` rise in temperature. If the generalisation holds for a reaction in the temperature range 295 K to 305 K, what would be the value of activation energy for the reaction?

Explanation

To find the activation energy (Ea) for the reaction, we can use the Arrhenius equation and the information given in the problem. Here’s a step-by-step solution:

### Step 1: Understand the Problem
We know that the rate of a chemical reaction doubles for every 10°C rise in temperature. We are given two temperatures: T1 = 295 K and T2 = 305 K. The corresponding rate constants are K1 and K2, where K2 = 2 K1.

### Step 2: Use the Arrhenius Equation
The Arrhenius equation relates the rate constant (K) to the temperature (T) and the activation energy (Ea):
\[ K = A e^{-\frac{E_a}{RT}} \]
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