An unusual atmospheric reaction leading to ozone destruction is CF₃O + O₃ → CF₃O₂ + O₂
The analysis of which has yielded an Arrhenius frequency factor (A) and activation energy of 2.0 × 10^-12 cm³ molecule^-1 s^-1 and 11.6 kJ/mol, respectively. Calculate the rate constant for this reaction at an altitude of 35 km, where the temperature is -34°C.

Question

Quizplus · Accepted Answer

The rate constant for the reaction can be calculated using the Arrhenius equation:

k = A e^(-Ea/RT)

where k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant (8.31 J/mol·K), and T is the temperature in Kelvin.

First, we need to convert the given activation energy from kJ/mol to J/mol:

Ea = 11.6 kJ/mol = 11,600 J/mol

The temperature in Kelvin can be calculated as follows:

T = -34°C + 273.15 = 239.15 K

Now we can plug in the given values and calculate the rate constant:

k = (2.0 × 10^-12 cm^3/molecule·s) e^(-11,600 J/mol / (8.31 J/mol·K × 239.15 K))
  = 3.5 × 10^-16 cm^3/molecule·s

Therefore, the best choice is C, which gives the closest value to the calculated rate constant.

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