Chem: Using Le Chatelier's principle, predict the direction of the net reaction in each of the following..?

A) 2 volumes reactants - 2 volumes of product - no change ↔

B) 1 volume reactant - 2 volumes product - increase pressure moves reaction to reactant side ←

c) 2 volumes reactant - 1 volume product - increase pressure moves reaction to products side.→

a)
N₂(g) + O₂(g) ⇌ 2NO(g)

In the equation, there are 2 moles of gaseous molecules on the left, while there are also 2 moles of gaseous molecules on the right. The number of gaseous molecules are equal on the both sides.

When pressure increases, according to Le Chatelier’s principle, the equilibrium position will be UNCHANGED.


====
b)
PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

In the equation, there is 1 mole of gaseous molecules on the left, while there are 2 moles of gaseous molecules on the right. There are a greater number of gaseous molecules on the right.

When pressure increases, according to Le Chatelier’s principle, the equilibrium position will shift to the LEFT in order to decrease the number of gaseous molecules.


====
c)
CO(g) + Cl₂(g) ⇌ COCl₂(g)

In the equation, there are 2 moles of gaseous molecules on the left, while there is 1 mole of gaseous molecules on the right. There are a greater number of gaseous molecules on the left.

When pressure increases, according to Le Chatelier’s principle, the equilibrium position will shift to the RIGHT in order to decrease the number of gaseous molecules.

a) N2(g) O2(g) ↔ 2NO(g)
There is no shift of the reaction. Due to equal number of moles on both sides. Effect of pressure causes no negligible change.


b) PCl5(g) ↔ PCl3(g) +Cl2(g)
High pressures favours the back-ward reaction and equilibrium shift towards the right to left side.


c) CO(g)+ Cl2(g) ↔ COCl2(g)
High pressure favours the forward reaction and equilibrium shift towards right hand side.