Two-point form of the Arrhenius Equation:
T1 = 25 ˚C + 273.15 = 298.15 K
T2 = 42.4 ˚C + 273.15 = 315.55 K
Given that the rate constant is 4.0×10−4 M-1 s-1 at 25.0 °C and that the rate constant is 2.6×10−3 M-1 s-1 at 42.4 °C, what is the activation energy in kilojoules per mole? Note that the value of the constant R is R = 8.3145 J/mol • K).
Express your answer numerically in kilojoules per mole using three significant figures.
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