Nitrous oxide decomposes exothermically into nitrogen and oxygen, at a temperature of approximately — Physical Chemistry — Kinetics Chemistry Question
Decomposition of Nitrous Oxide
Nitrous oxide decomposes exothermically into nitrogen and oxygen, at a temperature of approximately 565 °C.
2 N2O 2 N2(g) + O2(g)
This reaction follows the second-order kinetics when carried out entirely in the gas phase.
If the reaction is initiated with [N2O] equal to 0.108 mol dm-3, what will its concentration be after 1250 s have elapsed at 565 °C? The rate constant for the second order decomposition of N2O is 1.10×10-3 dm3 mol-1 s-1 at this temperature.
Model Answer
Because the reaction is second order, therefore
[N2O]t = 0.0940 mol dm-3
The activation energy for the second order reaction at 565 °C is 234 kJ mol-1. What is the rate constant for the reaction at 600 oC?
Model Answer
Using Arrhenius equation,
k2 = 4.23×10-3 dm3 mol-1 s-1