We’re being asked to determine the activation energy (Ea) of a reaction given that the plot of k vs. 1/T has a slope of –7445.
We’re given the plot of k (y) vs. 1/T (x).
This means we need to use the two-point form of the Arrhenius Equation:
k = rate constant
Ea = activation energy (in J/mol)
R = gas constant (8.314 J/mol • K)
T = temperature (in K)
A = Arrhenius constant or frequency factor
A plot of k versus 1/T has a slope of -7,445. What is E a, for this reaction?
A, 90.79 kJ/mol
B. 895.5 J/mol
C. 304.7 kJ/mol
D. 61.90 kJ/mol
E. 610.5 J/mol
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