The rates of most reaction double when their temperature is raised from `298K` to `308K`. Calculate their activation energy.

Explanation

To calculate the activation energy (Ea) when the rate of a reaction doubles as the temperature increases from 298 K to 308 K, we can use the Arrhenius equation in its logarithmic form. Here’s a step-by-step solution:

### Step 1: Understand the relationship between rate constants and temperature
When the temperature increases, the rate constant (K) of a reaction changes. In this case, we know that the rate doubles when the temperature rises from 298 K to 308 K. Therefore, we can express this as:
\[ \frac{K_2}{K_1} = 2 \]
where \( K_1 \) is the rate constant at 298 K and \( K_2 \) is the rate constant at 308 K.

### Step 2: Use the Arrhenius equation
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