For a certain reaction, the frequency factor A is 5.0 * 109 s-1 and the activation energy is 16.3 kJ/mol. What is the rate constant for the reaction at 79°C

K (79°C) = 1.906 E7 s-1

Explanation:

Arrhenius eq:

K (T) = A e∧ ( - Ea/RT)

∴ A = 5.0 E9 s-1

∴ Ea = 16.3 KJ/mol

∴ R = 8.314 E-3 KJ/K. mol

∴ T = 79°C ≅ 352 K ⇒ K = ?

⇒ K (79°C) = (5.0 E9 s-1) e∧[ - (16.3KJ/mol) / (8.314 E-3 KJ/K. mol) (352 K) ]

⇒ K (79°C) = (5.0 E9 s-1) e∧ ( - 5.5697)

⇒ K (79°C) = (5.0 E9 s-1) * (3.811 E-3)

⇒ K (79°C) = 1.906 E7 s-1