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The rate constant of a reaction is 1.2 x...

The rate constant of a reaction is `1.2 xx10^(-3) s^(-1)` at `30^@C` and `2.1xx10^(-3)s^(-1)` at `40^@C`. Calculate the energy of activation of the reaction.

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To calculate the energy of activation (Ea) for the reaction given the rate constants at two different temperatures, we can use the Arrhenius equation in its logarithmic form. Here’s a step-by-step solution: ### Step 1: Identify the given data - Rate constant at T1 (30°C): \( K_1 = 1.2 \times 10^{-3} \, \text{s}^{-1} \) - Rate constant at T2 (40°C): \( K_2 = 2.1 \times 10^{-3} \, \text{s}^{-1} \) - Temperature T1: \( 30°C = 303 \, K \) (converted to Kelvin) - Temperature T2: \( 40°C = 313 \, K \) (converted to Kelvin) ...
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