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)Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NH3 (g)delta 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)Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NH3 (g)delta H = -92 kJ/mol

kc_kennylau · Answer

@Callisto @ganeshie8 @nincompoop @Luigi0210 @Ashleyisakitty @shamil98 @myininaya

anonymous · Answer

is that all i write?

kc_kennylau · Answer

no

kc_kennylau · Answer

i'm not to familiar with the le chatelier's principle sorry

anonymous · Answer

When you have arrows going both ways this means the equation is at equilibrium. that as much as there are reactants crashing into each other to make products the products are also forming reactants. reactants r the left and products on the right. Now with the information of NH3 delta H-92. the heat is an endothermic reaction.. heat is be absorbed to create this product. if you increase the heat of this reaction it will favor the products because by le chateliers law an equilibrium equation will always want to go back to equilibrium. Also when pressure is applied only to Gaseous compounds pressure favors the side with least amount of moles.. So you have 4 moles total on the reactants vs 2 on the product.. so increasing pressure will favor the products as well.

anonymous · Answer

I think Studenttrainee is wrong. This reaction is exothermic not endothermicso it will be at low temperatures. His part about the pressure is correct.