Question

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?

Answer 1

Answer:

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