Help me solve question 7 i

Step 1: The equilibrium reaction is
$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \quad \Delta H = -92 \, kJ/mol$

Step 2: An increase in pressure is applied to the system at constant temperature.

Step 3: By Le Chatelier's principle, the equilibrium shifts to oppose the change and minimize the pressure increase.

Step 4: Total pressure depends on the number of moles of gas (at constant volume and temperature).
Formula: Shift favors the side with fewer moles of gas.

Step 5: Moles of gas:
Reactants: $1 \, (N_2) + 3 \, (H_2) = 4$ moles
Products: $2 \, (NH_3) = 2$ moles

Fewer moles on the product side.

Step 6: Equilibrium shifts to the right (forward), producing more $\mathrm{NH_3(g)}$ and reducing total moles from 4 to 2.

Effect: The equilibrium position shifts to the right, increasing the yield of ammonia ($\mathrm{NH_3}$).
Equilibrium shifts right (favors products)