How do increase in temperature and pressure affect the equilibrium of the following reaction: ${N_2}(g) + {H_2}(g) \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over{\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}$}} 2N{H_3}(g){\rm{ + Heat}}$

Question: How do increase in temperature and pressure affect the equilibrium of the following reaction: ${N_2}(g) + {H_2}(g) \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over{\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}$}} 2N{H_3}(g){\rm{ + Heat}}$

Solution:
Temperature:

The rate of the ammonia synthesis reaction increases with temperature. This is because the molecules have more energy at higher temperatures, which increases the probability of them colliding with enough energy to react. However, the equilibrium constant for the reaction decreases with temperature. This means that at higher temperatures, there is a smaller fraction of the reactants that are converted to products. As a result, the yield of ammonia decreases with increasing temperature.

Pressure:

The yield of ammonia increases with pressure. This is because the reaction is exothermic, meaning that it releases heat. As the pressure increases, the reaction shifts to the side that produces fewer moles of gas. In this case, the product side has one mole of gas, while the reactant side has three moles of gas. Therefore, as the pressure increases, more of the reactants are converted to products, and the yield of ammonia increases.