The Haber Process

Part of the Energy, Rates and Equilibrium section of Coddy's Chemistry journey. Lesson 31 of 35.

Haber: high pressure (about $200\ \mathrm{atm}$ ) favours ammonia.

$\mathrm{N_2(g)} + 3\mathrm{H_2(g)} \rightleftharpoons 2\mathrm{NH_3(g)} \qquad \Delta H = -92\ \mathrm{kJ}$

Low temperature favours ammonia but is too slow: about $450\ \mathrm{^{\circ}C}$ is the compromise.

The iron catalyst gives no shift and leaves K alone; equilibrium just comes sooner.

Challenge

A Haber plant switches to a new, more active iron catalyst:

$\mathrm{N_2(g)} + 3\mathrm{H_2(g)} \rightleftharpoons 2\mathrm{NH_3(g)} \qquad \Delta H = -92\ \mathrm{kJ}$

Which way does the equilibrium shift, and what happens to K?

Try it yourself

EquilibriumWhich way does it shift?

N₂(g)3 H₂(g)2 NH₃(g)

Test yourself

This lesson includes a short quiz. Start the lesson to answer it and track your progress.

All lessons in Energy, Rates and Equilibrium

1Energy in Reactions

4Rates of Reaction

7Practice Problems

2Bond Energies

5Equilibrium

3Changes of State

6Changing an Equilibrium