Use the reaction for the formation of NH3 from its elements N2(g) and H2(g) . This reaction has the following thermodynamic data:  ΔfHo (NH3) = - 45.9 kJ/mol and ΔfSo (NH3) = - 99.1 J/mol*K at 298 K a) Write a balanced equation (whole number ratios) for this process and write out the expression for the reaction quotient Q using partial pressures. b) Without doing any calculations, explain how the progression of the reaction will change (more reactants or more products) with respect to 1) increasing temperature, and 2) increasing pressure. c) Calculate the equilibrium constant K at 298 K d) Assuming that : ΔfHo  is independent of temperature, calculate K at - 78o C

Use the reaction for the formation of NH₃ from its elements N_2(g) and H_2(g) . This reaction has the following thermodynamic data:

 Δ_fH^o (NH₃) = - 45.9 kJ/mol and Δ_fS^o (NH₃) = - 99.1 J/mol*K at 298 K

a) Write a balanced equation (whole number ratios) for this process and write out the expression for the reaction quotient Q using partial pressures.

b) Without doing any calculations, explain how the progression of the reaction will change (more reactants or more products) with respect to 1) increasing temperature, and 2) increasing pressure.

c) Calculate the equilibrium constant K at 298 K

d) Assuming that : Δ_fH^o  is independent of temperature, calculate K at - 78^o C