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The activation energy of a chemical reaction can be calculated using the relationship between the rate constants at two distinct temperatures. Which of the following equations correctly represents this relationship?

1. log(k2/k1) = Ea/2.303R × [(T2 - T1)/(T1T2)]
2. log(k2/k1) = Ea/2.303R × [(T1 - T2)/(T1T2)]
3. log(k2/k1) = Ea/2.303R × [(T2 + T1)/(T1T2)]
4. log(k2/k1) = Ea/2.303R × [(T1 + T2)/(T1T2)]

Correct answer: log(k2/k1) = Ea/2.303R × [(T2 - T1)/(T1T2)]

Solution

The correct formula for determining activation energy is derived from the Arrhenius equation, and it matches option A. The term (T2 - T1)/(T1T2) correctly represents the temperature dependence of the rate constants.

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