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The reaction 2 NO2(g) → 2 NO (g) + O2(g) has rate constants of 2.70 x...

The reaction 2 NO2(g) → 2 NO (g) + O2(g) has rate constants of 2.70 x 10-2 M-1s-1 at 227 oC and 0.240 M-1s-1 at 277oC. What is the activation energy of this reaction? (Given: Arrhenius equation, k = Ae-Ea/RT )

A) 99.6 kJ/mol
B) 22.8 kJ/mol
C) 49.8 kJ/mol
D) -22.8 kJ/mol
E) 65.3 kJ/mol

I'm unsure on how to do it since you're not given the frequency factor

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