Question 1
The equilibrium between dinitrogen tetraoxide (colourless) and nitrogen dioxide (dark brown) is represented by the equation below:
N2O4(g) <-->2NO2(g) ∆H = +58kJ
- One mole of dinitrogen tetraoxide is placed in a22.4 dm3 glass container and allowed to equilibrate at 1000C under a pressure of 2.46 atm. Calculate the partial pressure of N2O4 ,NO2 and the equilibrium constant, Kc
- What would be observed if the temperature of the container is increased after equilibrium has established. Explain.