Problem: 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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FREE Expert Solution

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:



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

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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