We’re being asked to determine the activation energy of the reaction when the rate increases by 7.5x from 25°C to 30°C
This means we need to use the two-point form of the Arrhenius Equation:
k1 = rate constant at T1
k2 = rate constant at T2
Ea = activation energy (in J/mol)
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K).
Increasing the reaction temperature from 25°C to 30°C raises the reaction rate 7.5- fold. What is the activation energy?
A. 5.5 kJ
B. 303 kJ
C. 43.1 kJ
D. 16.2 kJ
E. 110. kJ
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