What type of deviation is shown by a mixture of ethanol and acetone?

A mixture of ethanol and acetone shows a positive deviation from Raoult's law. Raoult's law states that the partial vapor pressure of each component in an ideal solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution. In an ideal solution, the intermolecular forces between the components are similar. However, in a mixture of ethanol and acetone, the intermolecular forces between ethanol molecules (hydrogen bonding) and acetone molecules (dipole-dipole interactions) are stronger than the forces between ethanol and acetone molecules. This is because acetone cannot form hydrogen bonds as effectively as ethanol can. The weaker intermolecular forces between ethanol and acetone molecules lead to a higher vapor pressure than predicted by Raoult's law, resulting in a positive deviation. The solution's total vapor pressure is greater than the sum of the partial vapor pressures calculated using Raoult's law if the mixture were ideal. This results in a positive deviation because the escaping tendency of the molecules is greater than in an ideal solution.