Final answer:
The shift in equilibrium towards the products for the reaction N₂ (g) + 3H₂(g) → 2NH₃ (g) would occur with a decrease in temperature, a decrease in volume, removing some NH₃, and adding some N₂. The correct answer is option e, which is 2, 4, 5, 8.
Step-by-step explanation:
For the chemical equilibrium described by the equation N₂ (g) + 3H₂(g) → 2NH₃ (g) + 92.94 kJ, we analyze the factors that would cause a shift in the equilibrium towards products (to the right).
Decrease in temperature: Since the formation of NH₃ is exothermic (releases heat), decreasing the temperature would favor the forward reaction to produce more heat, thus shifting the equilibrium to the right. This corresponds to option 2.
Decrease in volume: A decrease in volume increases the pressure of the system. According to Le Chatelier's Principle, the system will shift towards the side with fewer moles of gas. Since the production of NH₃ results in fewer moles of gas compared to the reactants, a decrease in volume will shift the equilibrium to the right, which corresponds to option 4.
Remove some NH₃: Removing a product from the system will cause the equilibrium to shift to the right to produce more product, as per Le Chatelier's Principle, matching option 5.
Add some N₂: Adding more reactant (N₂) will cause the system to shift to the right to use up the excess reactant, corresponding to option 8.
The correct combination that will cause a shift to the right (towards products) is therefore 2, 4, 5, 8, which is option e from the multiple choices provided.