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:

∴ 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

the answer is a! (2.9 x 10^-18 j) hope i could someone. : )