Answer:
Q35 (C); Q36 (B)
Step-by-step explanation:
Li₃N + 2H₂ ⇌ 2LiNH₂ + 2LiH; ΔH° = -192 kJ·mol⁻¹
Q35. Reaction rate
The reaction is slow below because it has a high activation energy.
ΔH, ΔS, and ΔG determine the position of equilibrium and the spontaneity of the reaction, not its rate.
Q36. Maximizing amount of H₂
The reaction is exothermic. According to Le Châtelier's Principle, increasing the temperature will shift the position of equilibrium to the left and increase the amount of hydrogen.
Increasing the pressure will shift the position of equilibrium to the side with fewer moles of hydrogen.
Decreasing the pressure will shift the position of equilibrium to the side with more moles of hydrogen.
The correct answer is (B) increasing the temperature and decreasing the pressure .