Question 7. Explain the effect of the following on the equilibrium: N2(g) + 3H2(g) <=> 2NH3(g) (ΔH= -92kJ/mol) i. Increase in pressure:

Moles of gaseous reactants: $1~\mathrm{mol~N_2} + 3~\mathrm{mol~H_2} = 4~\mathrm{mol}$

Moles of gaseous products: $2~\mathrm{mol~NH_3} = 2~\mathrm{mol}$

Increasing pressure favors the direction with fewer moles of gas.

Here, products have fewer moles of gas ($2 < 4$).

The equilibrium shifts to the right (forward direction), producing more NH₃.

**Final answer: Equilibrium shifts right to produce more NH_3}