For the reaction below, describe the temperature and pressure conditions that would produce the highest yield for the forward reaction. Explain your answer in terms of Le Châtelier’s principle.

N2 (g) + 3 H2 (g) 2 NH3 (g) H = -92 kJ/mol

Question

For the reaction below, describe the temperature and pressure conditions that would produce the highest yield for the forward reaction. Explain your answer in terms of Le Châtelier’s principle. 

N2 (g) + 3 H2 (g)  2 NH3 (g) H = -92 kJ/mol

abb0t · Answer

The reaction is exothermic, which means that a low temperature will yeield a higher percentage. As far as pressure, I think that since it takes 4 moles to yield 2 moles of ammonia, I would say that the system opposes the volume decrease so a high pressure.

anonymous · Answer

The reaction is exotherm so the reaction must be occured at low temperature.
The number of mol at left side is greater than right side so the pressure must be high.

abb0t · Answer

That's exactly what I just said...