We’re being asked to determine the rate constant at 25°C of the reaction when k = 8.54 x 10-4 s -1 at 45°C with a EA = 90.8 kJ
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).
A reaction has a rate constant k = 8.54 x 10-4 s-1 at 45 °C and an activation energy, Ea = 90.8 kJ. What is the value of k at 25 °C?
A. 8.52 x 10-4 s-1
B. 4.46 x 10-3 s-1
C. 8.54 x 10-5 s-1
D. 4.46 x 10-4 s-1
E. 8.54 x 10-3 s-1
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