Hydrogen is produced industrially by the steam reforming of methane in a sealed container according to the following reversible reaction:
CH4(g)+H2O(g)⇌CO(g)+3H2(g)ΔH=+206 kJ mol−1 \text{CH}_4\text{(g)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO(g)} + 3\text{H}_2\text{(g)} \quad \Delta H = +206\text{ kJ mol}^{-1} CH4(g)+H2O(g)⇌CO(g)+3H2(g)ΔH=+206 kJ mol−1Which of the following combinations of changes would shift the position of equilibrium to the right?
Increasing the pressure and decreasing the temperature.
Decreasing the pressure and decreasing the temperature.
Decreasing the pressure and increasing the temperature.
Increasing the pressure and using a catalyst.