The rate constant of the reaction O + O₃ $\rarr$2O₂ is 7.0 × 10⁵ M^-1 s^-1 at -40°C and 4.8 × 10⁶ M^-1s^-1 at 25°C.Calculate the activation energy of this reaction.

Question

Quizplus · Accepted Answer

The activation energy can be calculated using the Arrhenius equation: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.Taking the natural logarithm of both sides of the equation, we get:ln(k) = ln(A) - (Ea/RT)Plotting ln(k) versus 1/T should give a straight line with a slope of -Ea/R.Using the given data, we can calculate the slope of the line:slope = (ln(4.8 × 10^6) - ln(7.0 × 10^5)) / ((1/298) - (1/233)) = -1.7 × 10^4 KTherefore, the activation energy is:Ea = -slope * R = -(-1.7 × 10^4 K) * 8.314 J/mol K = 17 kJ/mol

The Rate Constant of the Reaction O + O3 →\rarr→ 2O2 Is 7

The Rate Constant of the Reaction O + O₃ $\rarr$ 2O₂ Is 7