Problem: Dinitrogen tetraoxide, N 2O 4, decomposes to nitrogen dioxide, NO 2, in a first-order process. If k = 2.5 x 10 3 s -1 at 5 oC and k = 7.0 x 10 4 s -1 at 25°C, what is the activation energy for the decomposition?a. 214 kJ/molb. 361 kJ/molc. 323 kJ/mold. 115 kJ/mole. 151 kJ/mol

FREE Expert Solution

We’re being asked to determine the activation energy of the reaction when k = 2.5 x 10 3 s -1 at 5°C and k = 7.0 x 10 4 s -1 at 25°C


This means we need to use the two-point form of the Arrhenius Equation:


lnk2k1 = -EaR1T2-1T1


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

Dinitrogen tetraoxide, N 2O 4, decomposes to nitrogen dioxide, NO 2, in a first-order process. If k = 2.5 x 10 3 s -1 at 5 oC and k = 7.0 x 10 4 s -1 at 25°C, what is the activation energy for the decomposition?

a. 214 kJ/mol

b. 361 kJ/mol

c. 323 kJ/mol

d. 115 kJ/mol

e. 151 kJ/mol

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