Calculate the activation energy (Ea) in kJ/mol for a reaction. PLEASE HELP!

Question

Calculate the activation energy (Ea) in kJ/mol for a reaction if the rate constant (k) is 2.7 × 10^-4 (M^−1sec^−1) at 600 K and 3.5 × 10^−3 (M−^1sec^−1) at 650 K.

a. −166 kJ/mol
b. 166 kJ/mol
c. 1.64 kJ/mol
d. 1.66 × 10^5 kJ/mol

I really need help to understand this! Please show your work if possible, thanks in advance!

Answer 1

Hello Vivian,

 

To calculate the activation energy of a reaction, we use the Arrhenius equation.  You may want to look it up to see how and why it works.  In the problem you posted, there are two temperatures and two rate constants.  After some rearranging and substitution of the Arrhenius equation, we have

 

Ea = R T1 T2/(T1-T2) ln(k1/k2) = 8.314 J/mol K (600 K)(650 K)/(600 K-650 K) ln(2.7×10^-4 M^−1sec^−1/3.5×10^−3 M−^1sec^−1) = 166145 J/mol = 166 kJ/mol => choice b

 

All the best,

 

Randall

Answer 2

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