Deviations from Raoult’s law lead to the formation of azeotropes, constant boiling mixtures that cannot be separated by distillation, making industrial separations difficult. For components A and B, there is a positive deviation if the A-B attraction is less than A-A and B-B attractions (A and B reject each other), and a negative deviation if the A-B attraction is greater than A-A and B-B attractions. If the A-B attraction is nearly equal to the A-A and B-B attractions, the solution obeys Raoult’s law. Explain whether the behavior of each pair will be nearly ideal, have a positive deviation, or a negative deviation:(c) Hexane and heptane

Raoults Law defined as the non-volatile solute which contains the vapour pressure of solution is directly proportional to the mole fraction of the solvent.

The interaction between A- B is less than the interaction A- A and B-B interaction. Therefore, the escaping tendency of liquid molecules in mixture is greater than the escaping tendency in pure form. Hence, the vapour pressure of a mixture is greater than the initial value of vapour pressure.

The mixture of hexane and heptane show ideal deviation because it obeys Raoult's law at all pressure and temperature.

Thus from the above conclusion we can say that Hexane and heptane show nearly ideal behavior.

Learn more about the Ideal Deviation here: https://brainly.com/question/13208028

#SPJ4