What would be the energy of activation for a reaction when a change of temperature from `20^@C " to " 30^@C` exactly triples the reaction rate constant ?

Explanation

To determine the energy of activation (Ea) for a reaction when the temperature changes from 20°C to 30°C and the reaction rate constant triples, we can use the Arrhenius equation. Here’s a step-by-step solution:

### Step 1: Convert temperatures from Celsius to Kelvin
- The initial temperature (T1) is 20°C, which is converted to Kelvin as follows:
\[ T1 = 20 + 273 = 293 \, \text{K} \]
- The final temperature (T2) is 30°C, which is converted to Kelvin as follows:
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