For the reaction given below, the frequency factor A is 8.7 1012 s-1 and the activation energy is 63 kJ/mol. NO (g) + O3 (g) → NO2 (g) + O2 (g) What is the rate constant for the reaction at 70°C?

K (70°C) = 2213.376 s-1

Explanation:

balanced reaction:

NO (g) + O3 (g) → NO2 (g) + O2 (g)

∴ Ea = 63 KJ/mol

∴ A = 8.7 E12 s-1

∴ T = 70°C ≅ 343 K

Arrhenius eq:

K (T) = Ae∧ ( - Ea/RT)

∴ R = 8.314 E-3 KJ/K. mol

⇒ K (70°C) = (8.7 E12 s-1) e∧[ - (63) / (8.314 E-3) (343) ]

⇒ K (70°C) = (8.7 E12 s-1) * (2.5444 E-10)

⇒ K (70°C) = 2213.376 s-1