The activation energy for the reaction NO2(g)+CO(g)NO(g)+CO2(g) is E a = 375 kJ/

Question

The activation energy for the reaction NO2(g)+CO(g)NO(g)+CO2(g) is Ea = 375 kJ/mol and the change in enthalpy for the reaction is H = -375 kJ/mol .
What is the activation energy for the reverse reaction?

k=AeEa/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R=8.314 J/(molK) is the universal gas constant, and T is the absolute temperature. A certain reaction has an activation energy of 70.0 kJ/mol and a frequency factor of A1 = 4.00×1012 M1s1 . What is the rate constant, k, of this reaction at 24.0 C ?

An unknown reaction was observed, and the following data were collected:

T (K) k (M1s1)

352 109

426 185

Determine the activation energy for this reaction.

Explanation / Answer

1)

use:
delta H = Eaf - Ear
Eaf is activation energy of forward reaction
Ear is activation energy of reverse reaction

delta H = Eaf - Ear
-375 KJ/mol = 375 KJ/mol - Ear
Ear = 375 KJ/mol + 375 KJ/mol
= 750 KJ/mol

Answer: 750 KJ/mol

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