Draw a fully labelled diagram showing how a hydrogen bond forms between a water molecule and a methanol molecule.
Methanol has a melting point of $-97.6\,^\circ\text{C}$ and a boiling point of $64.7\,^\circ\text{C}$. A pure liquid methanol sample is placed in a flask, which is then sealed. After several days at constant temperature, the vapour pressure is measured to be $17\,\text{kPa}$. Describe the meaning of the term vapour pressure of methanol.
Explain why part of the liquid changes into a vapour.
Suggest and explain why the vapour pressure of water at room temperature is lower than the vapour pressure of methanol at room temperature. Refer to the correct intermolecular forces in your answer.
Methanol has a melting point of $-97.6^\circ\text{C}$ and a boiling point of $64.7^\circ\text{C}$. A pure liquid methanol sample is placed in a flask, which is then sealed. After several days at constant temperature, the vapour pressure is measured to be $17\,\text{kPa}$.
Methanol is produced by reacting carbon monoxide with hydrogen. $\text{CO}(g) + 2\text{H}_2(g) \rightleftharpoons \text{CH}_3\text{OH}(g)$ Carbon monoxide and hydrogen react at $1.0 \times 10^7\,\text{Pa}$ and $200^\circ\text{C}$. In time, the reaction mixture reaches dynamic equilibrium. The table gives the amounts of each species present in the mixture.
Explain what dynamic equilibrium means.
Calculate the partial pressure of methanol vapour at equilibrium under these conditions. Show your working.
Write an expression for the equilibrium constant, $K_p$, for this reaction. State the units in your answer.