Problem: A reaction has rate constant of 0.27 min-1 at 45 C and 0.90 min-1 at 55 C. What is the activation energy for the reaction (in kJ/mol)?A. -10.4B. 10.4C. 104D. 10,400E. 104,000

FREE Expert Solution

We’re being asked to determine the activation energy of the reaction when the rate increases from 0.27 min-1 to 0.90 min-1 at 45 to 55°C


This means we need to use the two-point form of the Arrhenius Equation:


lnk2k1 = -EaR1T2-1T1


where:

k1 = rate constant at T1 

k2 = rate constant at T

Ea = activation energy (in J/mol) 

R = gas constant (8.314 J/mol•K) 

T1 and T2 = temperature (in K).

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Problem Details

A reaction has rate constant of 0.27 min-1 at 45 C and 0.90 min-1 at 55 C. What is the activation energy for the reaction (in kJ/mol)?

A. -10.4

B. 10.4

C. 104

D. 10,400

E. 104,000

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