Midterm 2 - Question 3 | General Chemistry 3

Ammonia can be produced by the following reaction:

N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)

1) Calculate the value for ΔH⁰ for this reaction

2) Can the yield of ammonia be increased by raising the temperature? Justify

3) What is the equilibrium constant for the reaction?

4) If 235 mL of H₂ gas (25°C and 7.60 x 10⁴ Pa) were completely converted to ammonia and the ammonia were dissolved in water to make 0.500 L of solution, what would be the molarity of the resulting solution?

Data: At 298K:

ΔG⁰_f [NH₃ (g)] = - 33.0 kJ.mol^-1

S⁰ [N₂ (g)] = 191.5 J.mol^-1.K^-1

S⁰ [H₂ (g)] = 198.6 J.mol^-1.K^-1

S⁰ [NH₃ (g)] = 192.3 J.mol^-1.K^-1