DP Chemistry (last assessment 2024)

Question 22M.2.sl.TZ1.2c(i)

c(i).

[Maximum mark: 1]

22M.2.sl.TZ1.2c(i)

Ammonia, NH₃, is industrially important for the manufacture of fertilizers, explosives and plastics.

Ammonia is produced by the Haber–Bosch process which involves the equilibrium:

N₂(g) + 3 H₂(g) $⇌$ 2 NH₃(g)

(c(i))

Deduce the expression for the equilibrium constant, K_c, for this equation.

[1]

Markscheme

$K_{c} = \frac{{[N H_{3}]}^{2}}{[N_{2}] {[H_{2}]}^{3}}$ ✔

Examiners report

Most students could deduce the equilibrium constant expression from the equilibrium equation.

Syllabus sections