The reaction `C_(2)H_(5)I to C_(2)H_(4) + HI` is of first order and its rate constants are `3.20 xx 10^(-4) s^(-1)` at 600 K and `1.60 xx 10^(-2)s^(-1)` at 1200 K. Calculate the energy of activation for the reaction. (Given `R= 8.314 JK^(-1)mol^(-1))`

Explanation

To calculate the energy of activation (Ea) for the reaction \( C_2H_5I \to C_2H_4 + HI \), we can use the Arrhenius equation in the form:

\[ \ln K = -\frac{E_a}{R} \cdot \frac{1}{T} + \ln A \]

Where:
- \( K \) is the rate constant,
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