The rate of reaction triples when temperature changes form `20^(@)C` to `50^(@)C`. Calculate the energy of activation for the reaction `(R= 8.314JK^(-1)mol^(-1))`.

Explanation

To calculate the energy of activation for the reaction when the rate triples as the temperature changes from \(20^\circ C\) to \(50^\circ C\), we can use the Arrhenius equation. Here’s a step-by-step solution:

### Step 1: Convert temperatures to Kelvin
First, we need to convert the given temperatures from Celsius to Kelvin.
- \( T_1 = 20^\circ C + 273 = 293 \, K \)
- \( T_2 = 50^\circ C + 273 = 323 \, K \)

**Hint:** Remember that to convert Celsius to Kelvin, you add 273.
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