Question 22M.2.sl.TZ1.c(ii)
| Date | May 2022 | Marks available | [Maximum mark: 2] | Reference code | 22M.2.sl.TZ1.c(ii) |
| Level | sl | Paper | 2 | Time zone | TZ1 |
| Command term | Explain | Question number | c(ii) | Adapted from | N/A |
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)
Explain why an increase in pressure shifts the position of equilibrium towards the products and how this affects the value of the equilibrium constant, Kc.
[2]
shifts to the side with fewer moles «of gas»
OR
shifts to right as there is a reduction in volume✔
«value of » Kc unchanged ✔
Accept “Kc only affected by changes in temperature”.
Many students realised that increasing pressure shifts an equilibrium to the side with the most moles of gas (though the "of gas" was frequently omitted!) but probably less than half realised that, even though the equilibrium position changes, the value of the equilibrium constant remains constant.
