In industry, methanol is produced by reacting carbon monoxide with hydrogen. $\text{CO(g)} + 2\text{H}_2\text{(g)} \rightleftharpoons \text{CH}_3\text{OH(g)} \quad \Delta H = -90\ \text{kJ/mol}$ This process is normally conducted at a temperature of $400^\circ\text{C}$. Which row shows correctly how raising the temperature to above $400^\circ\text{C}$ affects both the equilibrium position and the reaction rate?
- Amoves to left; decreases
- Bmoves to left; increases
- Cmoves to right; decreases
- Dmoves to right; increases