Raoult’s Law and Ideal Solutions Quiz

Mole fraction of the non-volatile solute

Ideal solutions

Positive deviations and negative deviations

$P_{total} = p_{1}^{0}x_{1} + p_{2}^{0}x_{2}$

Mole fraction of the non-volatile solute

Raoult's Law = The law stating that the relative lowering of the vapour pressure of the solvent in a solution is equal to the mole fraction of a non-volatile solute Ideal Solutions = Solutions that obey Raoult's law over the entire range of concentrations Positive deviations = Types of deviations from Raoult's law where the actual vapour pressure is higher than predicted by Raoult's law Negative deviations = Types of deviations from Raoult's law where the actual vapour pressure is lower than predicted by Raoult's law

Vapour pressure lowering in a solution = Ruled by Raoult's Law which relates it to the mole fraction of a non-volatile solute Ptotal= p10x1+p20x2 = Expression used to represent Raoult's Law in terms of partial pressures and mole fractions Ideal solution characteristics = Solutions that follow Raoult's Law throughout all concentrations Deviation types = Categories including positive and negative deviations from Raoult's Law

Positive deviations = When the observed vapour pressure is higher than predicted by Raoult’s law Negative deviations = When the observed vapour pressure is lower than predicted by Raoult’s law Ideal Solutions = Solutions that obey Raoult’s law over the entire range of concentrations Raoult’s Law = States that the relative lowering of the vapour pressure of the solvent over a solution is equal to the mole fraction of a non-volatile solute present in the solution

Ptotal= p10x1+p20x2 = Expression used to represent Raoult’s Law Vapour Pressure = The pressure exerted by a vapour in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system Mole Fraction = The ratio of the number of moles of a component in a mixture to the total number of moles in the mixture Solvent = The substance that dissolves the solute to form a solution

Non-volatile solute = Does not easily evaporate at normal temperatures Ideal Solutions = Obey Raoult’s law over the entire range of concentrations Solvent = The component present in larger quantity in a solution Mole Fraction = Represents the ratio of moles of one component to the total moles in a solution

Raoult’s Law = States that the relative lowering of vapour pressure is proportional to the mole fraction of solute present Vapour Pressure = Pressure exerted by a vapour in equilibrium with its condensed phases at a specific temperature Mole Fraction = Ratio of moles of a component to total moles in a mixture Positive Deviations = When observed vapour pressure is higher than predicted by Raoult’s Law

Raoult’s Law = Relates lowered vapour pressure to solute concentration in solution Ideal Solutions = Solutions that perfectly follow Raoult’s Law at all concentrations Negative Deviations = Occurs when observed vapour pressure is less than expected by Raoult’s Law Mole Fraction = Expresses component concentration relative to total moles in a solution