This question is about the industrial methanation equilibrium:
CO(g)+3H2(g)⇌CH4(g)+H2O(g)\text{CO}(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_4(\text{g}) + \text{H}_2\text{O}(\text{g})CO(g)+3H2(g)⇌CH4(g)+H2O(g)
State and explain the effect, if any, of an increase in overall pressure on the equilibrium yield of CH4\text{CH}_4CH4.
A 0.600 mol0.600\text{ mol}0.600 mol sample of CO\text{CO}CO is mixed with a 1.600 mol1.600\text{ mol}1.600 mol sample of H2\text{H}_2H2 in a sealed container at a constant temperature. When equilibrium is reached at a total pressure of 280 kPa280\text{ kPa}280 kPa, the mixture contains 0.400 mol0.400\text{ mol}0.400 mol of CH4\text{CH}_4CH4.
Calculate the partial pressure, in kPa\text{kPa}kPa, of CO\text{CO}CO in this equilibrium mixture.
A different mixture of CO\text{CO}CO and H2\text{H}_2H2 reaches equilibrium at a different temperature. The table below shows the partial pressures of the gases at equilibrium:
| Gas | Partial pressure / kPa\text{kPa}kPa |
|---|---|
| CO\text{CO}CO | 1.20×1021.20 \times 10^21.20×102 |
| H2\text{H}_2H2 | 2.00×1022.00 \times 10^22.00×102 |
| CH4\text{CH}_4CH4 | 8.00×1018.00 \times 10^18.00×101 |
| H2O\text{H}_2\text{O}H2O | 6.00×1016.00 \times 10^16.00×101 |
Give an expression for the equilibrium constant (KpK_pKp) for this reaction. Calculate the value of the equilibrium constant for this reaction and give its units.
What is the effect on the value of KpK_pKp if the pressure of this equilibrium mixture is increased at a constant temperature?
Select one option: