We’re being asked to determine the rate constant of the reaction at 720.0 K.
We’re given the rate constant at another temperature and the activation energy of the reaction.
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).
The following reaction has an activation energy of 262 kJ/mol.
C4H8(g) → 2C2H4(g)
At 600.0 K, the rate constant is 6.1 x 10 -8 s-1.
What is the value of the rate constant at 720.0 K.
K= ? answer in s-1
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