Calculate K_p for each reaction.
b. N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) K_c = 3.7⨉10⁸ (at 298 K)
c. N₂(g) + O₂(g) ⇌ 2 NO(g) K_c = 4.10⨉10^-31 (at 298 K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. Kc refers to concentrations in molarity, while Kp refers to partial pressures. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In the given reaction, N2(g) + 3H2(g) ⇌ 2NH3(g), the stoichiometric coefficients indicate that one mole of nitrogen reacts with three moles of hydrogen to produce two moles of ammonia. This stoichiometry is crucial for calculating changes in concentrations or pressures at equilibrium.

The equilibrium constant Kp is temperature-dependent, meaning its value changes with temperature. For exothermic reactions, Kp decreases with increasing temperature, while for endothermic reactions, Kp increases. Understanding this dependence is essential when calculating Kp at a specific temperature, as it directly influences the equilibrium position and the concentrations of reactants and products.