We’re being asked to determine the rate constant at 795.0 K. We are asked for rates at two different temperatures.
This means we need to use the two-point form of the Arrhenius Equation:
where 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)
The following reaction has an activation energy of 262 kJ/mol.
C4H8 (g) → 2 C2H4 (g)
At 600.0 K the rate constant is 6.1x 10-8 s-1. What is the value of the rate constant at 795.0 K?
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