Chemistry Solutions and Equilibrium Concepts

Describes the behavior of mixtures where one component is uniformly distributed throughout another.

Solutions that obey Raoult's Law, meaning the vapor pressure of a solution is directly proportional to the mole fraction of the solvent.

Solutions that deviate from Raoult's Law, exhibiting non-ideal behavior due to interactions between solute and solvent.

Properties of solutions that depend on the concentration of solute particles, not their identity.

The study of chemical reactions that proceed in a reversible manner, involving both forward and reverse reactions.

A mixture with a uniform composition and properties throughout.

A mixture with non-uniform composition and properties. Different parts of the mixture have different characteristics.

The substance present in a solution in a larger amount.

The substance present in a solution in a smaller amount that dissolves in the solvent.

A solution that has reached its maximum saturation point. No more solute can be dissolved at that temperature.

A solution that contains less solute than the maximum it can hold at that temperature.

A solution that temporarily holds more solute than it normally can at that temperature. It's unstable and can easily precipitate out excess solute.

Solutions containing charged particles, such as ions, that interact electrostatically. They conduct electricity.

A thermodynamic property that describes the free energy per mole of a species in a mixture. It indicates the tendency of a substance to move or react.

A closed system where the total mass and energy remain constant. No matter is exchanged with the surroundings.

Describes the amount of a substance present in a mixture, expressed as a fraction of the total moles of all components in the mixture.

The change in chemical potential of a species in a mixture compared to its pure state. It reflects the deviation from ideal behavior.

The total Gibbs Free Energy of a mixture is the sum of the chemical potential of each component multiplied by its mole fraction.

The Gibbs Free Energy of a mixture is the sum of the chemical potential of each component multiplied by its mole fraction.

A measure of the tendency of a substance to move from a pure state to a mixed state. It reflects the differences in molecular interactions between the pure substance and the mixture.

The sum of the partial mole fractions of all components in a mixture must equal 1. This signifies that the system consists of all components present.

A mathematical equation used to calculate the vapor pressure of a liquid at a given temperature, considering its heat of vaporization.

The amount of energy required to convert one mole of a liquid into its gaseous state at constant pressure.

The pressure exerted by the vapor of a liquid in equilibrium with its liquid phase at a given temperature.

A measure of the attractive forces between molecules in a liquid.

A law stating that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent.

The difference in chemical potential for a species at a given temperature is determined by its activity, which is a measure of its effective concentration in the mixture. For a perfect gas, the chemical potential is related to its partial pressure.

The tendency of a substance to evaporate from its liquid phase.

At equilibrium, the change in Gibbs free energy for a reaction is zero. This means the free energy of the reactants and products are equal, indicating no net change in the system.

For a physical transition, like vaporization, the chemical potentials of a substance in its two phases must be equal. The overall change in Gibbs free energy for the transition must be negative for it to occur.

If a liquid is placed in an evacuated container, some will evaporate until equilibrium is reached. The pressure of the vapor at equilibrium is called the vapor pressure, and it is a characteristic property of the liquid. It increases rapidly with temperature.

The temperature at which the vapor pressure of a liquid equals 1 atmosphere is called its normal boiling point. This is the temperature at which the liquid transforms into a gas.

Some solids can have a measurable vapor pressure even at room temperature. If the vapor pressure reaches 1 atmosphere below the melting point, the solid sublimes directly into a gas. This temperature is called the normal sublimation point.

The boiling point and sublimation point are affected by the external pressure. Higher pressure requires a higher temperature for these transitions to occur.

Even at low temperatures, some molecules in a liquid have enough energy to escape the liquid's cohesive forces and vaporize. This leads to the rapid increase in vapor pressure with increasing temperature.

The rate of evaporation of a pure solvent is directly proportional to the surface area, with a rate constant 'kevap'.

The rate of condensation of a pure solvent is directly proportional to the partial pressure of the solvent in the gas phase, with a rate constant 'kcond'.

For a pure solvent, the equilibrium vapor pressure is reached when the rate of evaporation equals the rate of condensation.

For an ideal solution, the equilibrium vapor pressure of the solvent is reduced by a factor equal to the mole fraction of the solvent in the solution.

The chemical potential of a pure component 'i' in the gas phase at standard pressure 'Po' is equal to 'μ° + RTln(Po)', where 'μ°' is the standard chemical potential of 'i' at 'Po'.

The chemical potential of a pure liquid component 'i' is equal to 'μ° + RTln(P°i)', where 'P°i' is the vapor pressure of 'i' in the pure state.

The change in Gibbs free energy of an ideal solution during mixing is zero, meaning the mixing process is spontaneous.