Methanol (CH3OH\text{CH}_3\text{OH}CH3OH) is manufactured industrially from synthesis gas, which is a mixture of carbon monoxide and hydrogen.
The reaction is reversible and reaches 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 industrial process is typically operated at a pressure of about 50 to 100 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 vapor and oxygen is passed over a heated copper catalyst. Methanal and water are the only 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 fuel. Write the chemical equation for the complete combustion of methanol.
