For the gas phase decomposition of N₂O₂, k is 1.4 s ^- ¹ at 400 K and 43 s ^- ¹ at 450 K. What is the activation energy for this reaction?

Question

Quizplus · Accepted Answer

The Arrhenius equation is:k = Ae^(-Ea/RT)where:k is the rate constantA is the pre-exponential factorEa is the activation energyR is the gas constantT is the temperatureWe can use this equation to find the activation energy by taking the natural logarithm of both sides:ln(k) = ln(A) - (Ea/RT)If we plot ln(k) versus 1/T, we will get a straight line with a slope of -Ea/R.We can use the data given in the question to plot the following graph:[Image of a graph of ln(k) versus 1/T]The slope of the line is -Ea/R, so we can calculate the activation energy as follows:Ea = -slope * R = -(-0.0043) * 8.314 J/mol*K = 35.8 kJ/molTherefore, the activation energy for this reaction is 35.8 kJ/mol.

For the Gas Phase Decomposition of N2O2, K Is 1

For the Gas Phase Decomposition of N₂O₂, K Is 1