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What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20°C to 35°C (R = 8.314 J mol⁻¹ K⁻¹)?

1. 269 kJ mol⁻¹
2. 34.7 kJ mol⁻¹
3. 15.1 kJ mol⁻¹
4. 342 kJ mol⁻¹

Correct answer: 34.7 kJ mol⁻¹

Solution

The relationship between rate and temperature is given by the Arrhenius equation. Using the formula ln(k2/k1) = (Ea/R) * [(T2 - T1) / (T1 * T2)], substituting the given values, and solving for Ea, we find it to be approximately 34.7 kJ mol⁻¹.

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