The industrial synthesis of methanol is a reversible reaction that reaches an equilibrium :
CO(g)+2H2(g)⇌CH3OH(g) \text{CO}(\text{g}) + 2\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g}) CO(g)+2H2(g)⇌CH3OH(g)The forward reaction is exothermic.
The rate of attainment of equilibrium and the equilibrium yield of methanol are affected by pressure, temperature, and the presence of a catalyst.
A chemical manufacturer considered two sets of reaction conditions, X and Y.
In both setups, carbon monoxide is mixed with excess hydrogen.
Only setup Y utilizes a catalyst, along with a lower temperature and higher pressure than setup X.
The conditions for X and Y are summarized in the table below:
| Set of conditions | Pressure in atm | Temperature in °C | Catalyst |
|---|---|---|---|
| X | 50 | 380 | No catalyst used |
| Y | 100 | 250 | Copper-based catalyst used |
The manufacturer chose to operate using set of conditions Y rather than set of conditions X.
Explain, by considering the effect of changing these conditions on both the rate of attainment of equilibrium and on the equilibrium yield of methanol, why the manufacturer chose set of conditions Y.
Practise Edexcel GCSE Chemistry Reversible reactions and equilibria with exam-style questions for Foundation and Higher tier. 38 questions, matched to the Edexcel GCSE Chemistry (1CH0) specification and written in Paper 1 and Paper 2 style. Every question includes a full worked solution and mark scheme, so you can see where marks are awarded rather than just whether you got the answer right.
