Ethanol has a boiling point of $78^\circ\text{C}$. When the pressure is $101\ \text{kPa}$ and the temperature is $79^\circ\text{C}$, ethanol vapour does not obey the gas equation $pV = nRT$ exactly. What is the reason for this?
- AEthanol vapour is in equilibrium with ethanol liquid at $79^\circ\text{C}$.
- BThere are intermolecular forces between the molecules of ethanol vapour.
- CThe vapourisation of ethanol liquid is an endothermic process.
- DVapours will not obey the gas equation perfectly at such a low pressure.