Help me solve question 7 i

Physics

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Step-by-step solution

6 steps

  1. The equilibrium reaction is

    N2(g)+3H2(g)⇌2NH3(g)ΔH=−92 kJ/mol\mathrm{N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)} \quad \Delta H = -92 \, \mathrm{kJ/mol}

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

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

  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.

  5. Moles of gas

    Reactants: 1 (N2)+3 (H2)=41 \, (\mathrm{N_2}) + 3 \, (\mathrm{H_2}) = 4 moles
    Products: 2 (NH3)=22 \, (\mathrm{NH_3}) = 2 moles

    Fewer moles on the product side.

  6. Equilibrium shifts to the right (forward), producing more NH3(g)\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 (NH3\mathrm{NH_3}).
    Equilibrium shifts right (favors products)

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