Select correct answer(s) that would yield more products in the following reaction.
CH₄(g) + 4 F₂(g) ⇌ CF₄(g) + 4 HF(g) ΔH = 38.2 kJ/mol
a) increase pressure
b) increase temperature
c) add 0.31 moles of F₂
d) add some Xenon gas
e) cool down reaction vessel
f) decrease volume

• A. a and d
• B. a and e
• C. b and c
• D. b and e
• E. a, d and e
• F. b, c, and f

Answer: (C)

Verified step by step guidance

1. Identify the reaction and its characteristics: The reaction is CH\_4(g) + 4 F\_2(g) ⇌ CF\_4(g) + 4 HF(g) with ΔH = +38.2 kJ/mol, indicating it is endothermic (absorbs heat).
2. Apply Le Chatelier's Principle to temperature changes: Since the reaction is endothermic, increasing temperature will shift the equilibrium toward the products to absorb the added heat, thus producing more products.
3. Analyze the effect of changing reactant concentration: Adding more F\_2 (a reactant) will shift the equilibrium toward the products to consume the added reactant, increasing product formation.
4. Consider pressure and volume changes: Count moles of gas on each side (reactants: 1 + 4 = 5 moles; products: 1 + 4 = 5 moles). Since moles of gas are equal on both sides, changing pressure or volume will not favor either side significantly.
5. Evaluate the effect of inert gases (like Xenon): Adding an inert gas at constant volume does not change partial pressures of reactants or products, so it does not shift the equilibrium or increase product formation.