The high temperatures in an automobile engine cause nitrogen and oxygen to form noxious nitrogen monoxide. Use the following data on the temperature dependence of the rate constant to determine the activation energy for this reaction.

Question

Quizplus · Accepted Answer

Using the Arrhenius equation, we can calculate the activation energy (Ea) using two sets of temperature and rate constant (k) data. Let's choose the data at 1,800 K and 2,400 K:

ln(k2/k1) = -(Ea/R)((1/T2)-(1/T1))

ln(2.1x10^-15/6.3x10^-17) = -(Ea/8.314)((1/2400)-(1/1800))

ln(33.33) = -(Ea/8.314)(0.000413)

Ea = -ln(33.33)/(0.000413*8.314) = 310 kJ/mol

Therefore, the activation energy for this reaction is 310 kJ/mol, which corresponds to choice D.

The High Temperatures in an Automobile Engine Cause Nitrogen and Oxygen