Question

The reaction 2NOCl(g) → 2NO(g) + Cl₂(g) has a rate constant of 9.1×10⁻⁶ s-1 at 75.2°C and 6.7×10⁻⁴ s⁻¹ at 124.8°C. Determine the activation energy for this reaction to the nearest whole number in units of kilojoules per mole.

Answer 1

The activation energy for the reaction is approximately 58 kJ/mol.

Step-by-step explanation:

The rate constant of a reaction depends on temperature according to the Arrhenius equation. The Arrhenius equation is given by:

k = Ae-Ea/RT

where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin. By rearranging the equation, we can solve for Ea:

Ea = -RT(ln(k/A))

Using the given rate constants and temperatures, we can calculate the activation energy for this reaction:

Ea = -8.314 J/mol·K * (ln((6.7x10^-4)/(9.1x10^-6))) = 58000 J/mol ≈ 58 kJ/mol

Learn more about activation energy