Carbon monoxide and hydrogen are used in the industrial synthesis of methanol (CH3OH\text{CH}_3\text{OH}CH3OH).
The reaction is reversible and can reach a position of dynamic equilibrium.
CO(g)+2H2(g)⇌CH3OH(g)ΔH=−91 kJ/mol \text{CO}(\text{g}) + 2\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g}) \qquad \Delta H = -91 \text{ kJ/mol} CO(g)+2H2(g)⇌CH3OH(g)ΔH=−91 kJ/molThe reaction is typically carried out at a pressure of about 80 atmospheres and a temperature of 250∘C250^\circ\text{C}250∘C.
State two features of a reaction that is in dynamic equilibrium.
How would a decrease in temperature at constant pressure affect the amount of methanol in the equilibrium mixture? Explain your answer.
How would an increase in pressure at constant temperature affect the amount of methanol in the equilibrium mixture? Explain your answer.
Methanol (CH3OH\text{CH}_3\text{OH}CH3OH) can be converted into methanal (HCHO\text{HCHO}HCHO). A mixture of methanol and oxygen is passed over a heated silver catalyst. Methanal and water are the only two products.
Write a chemical equation for this conversion of methanol into methanal.
What is meant by the term catalyst?
Explain how a catalyst works.
Methanol can be used as a liquid biofuel. Write the chemical equation for the complete combustion of methanol.
