What is the activation energy of a chemical reaction if the reaction rate triples when the temperature goes from 10$^{\circ}$C to 30$^{\circ}$C? A) 5.5 $\times$ 10^-20 J B) 6.0 $\times$ 10^-20 J C) 6.5 $\times$ 10^-20 J D) 7.0 $\times$ 10^-20 J E) 7.5 $\times$ 10^-20 J

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Quizplus · Accepted Answer

The activation energy can be calculated using the equation ln(k2/k1) = (-Ea/R)(1/T2 - 1/T1), where k1 and k2 are the rate constants at the two temperatures, T1 and T2. Since the rate triples, k2 = 3k1. Converting the temperatures to Kelvin gives T1 = 283 K and T2 = 303 K. Substituting these values and solving for Ea gives Ea = 6.5*10^4 J/mol. Therefore, the answer is C.

What Is the Activation Energy of a Chemical Reaction If ∘^{\circ}∘

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