PCl5 (g) ↔ PCl3 (g) + Cl2 (g) DH0 = 87.9 kJ
How will the following affect the above equilibrium?
a) increasing the concentration of PCl5
Equilibrium position shifts to the right. PCl5=decreases PCl3 and CL2 increases.
b) decreasing the concentration of Cl2
Equilibrium position shifts to the right. PCl5=decreases CL2 increases.
c) increasing the temperature would cause the reaction to favour the endothermic reaction ( which is the favoured reaction) to minimise change in temperature.
d) Increasing the size of the reaction vessel would cause the pressure to decrease. There are more moles of gas on the RHS of the equation. So the equilibrium position shifts to the right to make more moles of gas so that the pressure doesn’t change when the vessel size is increased.
e) adding a catalyst wouldn’t affect the equilibrium position