State what Le Chatelier’s Principle says.
Using your knowledge of Le Chatelier’s Principle, state the temperature and pressure conditions that could be used to produce a greater yield of methanol in this process. For each condition, explain why the yield would rise.
The carbon monoxide used to make methanol may be produced by reacting carbon dioxide with hydrogen. $$\text{CO}_2\text{(g)} + \text{H}_2\text{(g)} \rightleftharpoons \text{CO(g)} + \text{H}_2\text{O(g)}$$ $$K_c = 1.44\ \text{at}\ 1200\ \text{K}$$ A mixture containing $0.70\ \text{mol}$ of $\text{CO}_2$, $0.70\ \text{mol}$ of $\text{H}_2$, $0.30\ \text{mol}$ of $\text{CO}$ and $0.30\ \text{mol}$ of $\text{H}_2\text{O}$ was put into a $1\ \text{dm}^3$ flask and left to reach equilibrium at $1200\ \text{K}$. Calculate the amount, in moles, of each substance in the equilibrium mixture at $1200\ \text{K}$.