In the Haber process, nitrogen gas reacts with hydrogen gas to form gaseous ammonia (see Problem 14.76).

(a) Write the equilibrium expression for the reaction.

(b) The equilibrium constant at a certain temperature is 1.5 × 10^–2. If the equilibrium concentrations of hydrogen and nitrogen are both 0.20 M at this temperature, what is the equilibrium concentration of ammonia?

Data from Problem 14.76

Suppose you are making ammonia (NH₃) by the Haber reaction, at 472 °C:

Describe qualitatively where the equilibrium lies for this reaction.

On the face of it, would this reaction be a good one for isolating pure ammonia?

What would happen if you could keep feeding H₂ and N₂ into the reaction vessel while at the same time removing NH₃?

Transcribed Image Text:

3 H₂(8) + N₂(8) ⇒ 2 NH3(8) Keq = 0.105