Problem: 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?

FREE Expert Solution

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:


ln k2k1=-EaR[1T2-1T1]


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)


92% (368 ratings)
View Complete Written Solution
Problem Details

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?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Arrhenius Equation concept. You can view video lessons to learn Arrhenius Equation. Or if you need more Arrhenius Equation practice, you can also practice Arrhenius Equation practice problems.