This question is about the reaction: N 2 (g) + 3H 2 (g) 2NH 3 (g)

Question:

This question is about the reaction:

N₂(g) + 3H₂(g) ⇌ 2NH₃(g) ΔH_r = –92 kJ mol^–1

120.0mol of hydrogen gas are mixed with 40.0mol of nitrogen gas then pressurised. The mixture of gases is passed at constant pressure over an iron catalyst at 450°C until the mixture reaches equilibrium. The total volume of the mixture is 1.0 dm³. 20% of the reactants are converted to ammonia.

a. How many moles of nitrogen and hydrogen remain at equilibrium?

b. How many moles of ammonia are formed?

c. Write an equilibrium expression for K_c.

d. Calculate a value for K_c, including units.

e. What will happen to the numerical value of K_c when the pressure is raised?

f. What will happen to the numerical value of K_c when the temperature is raised?

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