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

Step 1: Write the given equilibrium equation.

Step 2: Calculate moles of gaseous reactants and products.

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

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

Step 3: Apply Le Chatelier's principle to an increase in pressure.

Increasing pressure favors the direction with fewer moles of gas.

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

Step 4: Predict the effect.

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

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