Carbon reacts with hydrogen in a closed reactor at constant temperature.
C(s)+2H2(g)⇌CH4(g) \mathrm{C(s) + 2H_{2}(g) \rightleftharpoons CH_{4}(g)} C(s)+2H2(g)⇌CH4(g)The table shows the percentage of hydrogen converted to methane when equilibrium is reached.
| Pressure in kPa | Hydrogen converted to methane in % |
|---|---|
| 100 | 35 |
| 300 | 52 |
| 600 | 66 |
Explain the trend in the data as the pressure increases. Use the equation in your answer.
Methane is continuously removed from the reaction mixture as it forms.
Explain how this affects the total amount of methane made.
124 exam-style questions on OCR GCSE Chemistry 5.3 Equilibria, covering 5.3.1 Reversible reactions and dynamic equilibrium and 5.3.2 Changing the position of equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.