Answer to Question #331308 in Organic Chemistry for vin

Question

A reaction has a rate constant of 7.3x10 M/s at 315 K and a frequency factor of 4.4x10 What is the activation energy of the reaction?

Answer 1

Solution:

Activation energy of the reaction can be calculated from Arrhenius equation

k = A × e^−(Ea/RT)

where,

k = chemical reaction rate

A = frequency factor

E_a = activation energy

R = gas constant

T = temperature

k = 7.3×10⁻⁴ M s⁻¹

A = 4.4×10⁷ M s⁻¹

E_a = ???

R = 8.314 J mol⁻¹ K⁻¹

T = 315 K

Thus,

(7.3×10⁻⁴) = (4.4×10⁷) × e^{−Ea / (8.314 × 315)}

1.659×10⁻¹¹ = e^{−Ea × 0.0003818}

ln(1.659×10⁻¹¹) = −E_a × 0.0003818

−24.8222 = −E_a × 0.0003818

E_a = 65013.67 J mol⁻¹ = 6.5×10⁴ J mol⁻¹

E_a = 6.5×10⁴ J/mol

Answer: The activation energy of the reaction is 6.5×10⁴ J/mol