CHAPTER 6: Chemical Equilibria

 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 dmglass container and allowed to equilibrate at 1000C under a pressure of 2.46 atm. Calculate the partial pressure of N2O4 ,NOand the equilibrium constant, Kc
  • What would be observed if the temperature of the container is increased after equilibrium has established. Explain.