Much of the brown haze hanging over large cities is nitrogen dioxide, NO2(g). Nitrogen dioxide reacts to form dinitrogen tetroxide, N2O4(g), according to the equilibrium.

Question

2NO2(g) N2O4(g) + 57.2 kJ

(brown) (coulorless)

Use this equilibrium to explain why the brownish haze over a large city dissapears in the winter , only to reappear again in the spring.(Assume that the atmosphere over a city constitutes a closed system.)

Answer 1

The following reaction is used in the commercial production of hydrogen gas.

CH4(g) + 2H2O(g) CO2(g) + 4H2(g)

a) In a closed system how would a catalyst affect the establishment of equilibrium in the system?
b) How would the concentration of H2(g) at equilibrium be affected by the use of a Ni(s) catalyst?

Answer 2

It's tough to follow when you post a question as a piggy back to another question. Most of the times they get lost in the shuffle. Please post a new question for new questions.

Answer 3

2NO2(g) N2O4(g) + 57.2 kJ
Adding heat, as in the summer, will push the equilibrium to the left forming more NO2 and more color. (N2O4 is colorless). The winter takes away heat and the equilibrium shifts to the right.