Recall: The Arrhenius equation gives us the relationship of the rate constant k with temperature and activation energy Ea. The two-point form of the Arrhenius equation is:
k1 = 2.45 × 10–4 L/mol•s T1 = 302 ˚C + 273.15 = 575.15 K
k2 = 0.891 L/mol•s T2 = 508°C + 273.15 = 781.15 K
Consider the hypothetical reaction A 2 (g) + B2 (g) → 2AB (g), where the rate law is:
The value of the rate constant at 302°C is 2.45 x 10 -4 L/mol•s, and at 508°C the rate constant is 0.891 L/mol•s. What is the activation energy for this reaction? What is the value of the rate constant for this reaction at 375°C?
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