CHEM TERMSKinetic Molecular Theory of Gases - Gas particles move in constant, random, and straight-line motion. They are widely spaced, collide with each other and container walls, and act independently. Physical Properties of Gases - Gases expand to fill

Kinetic Molecular Theory of Gases

Gas particles move in constant, random, and straight-line motion. They are widely spaced, collide with each other and container walls, and act independently.

Physical Properties of Gases

Gases expand to fill containers, are fluids, have low densities, can be compressed, and undergo diffusion and effusion.

Atmospheric Pressure

The force exerted by air on a given volume, measured by a barometer or manometer.

Evangelista Torricelli

Scientist who developed the barometer to measure atmospheric pressure.

Standard Temperature & Pressure (STP)

0℃ (273.15 K), 1 atm (101.325 kPa), and a standard volume of 22.414 L.

Boyle's Law

At constant temperature, the volume of a gas is inversely proportional to pressure.

Charles' Law

The volume of a confined gas is directly proportional to temperature when pressure is constant.

Gay

Lussac's Law - The pressure of a confined gas is directly proportional to temperature when volume is constant.

Graham's Law of Diffusion

The rate of diffusion of a gas is inversely proportional to the square root of its molar mass.

Dalton's Law of Partial Pressures

The total pressure of a gaseous mixture is equal to the sum of the partial pressures of its components.

Combined Gas Law

The volume of a gas is proportional to absolute temperature divided by pressure.

Avogadro's Law

The volume of a gas is directly proportional to the number of moles at constant temperature and pressure.

Ideal Gas Law

Describes the relationship among volume, pressure, temperature, and the number of moles of a gas.

Gas Stoichiometry

The study of quantitative relationships between reactants and products in gas-phase reactions.

Solution

A homogeneous mixture composed of a solute and a solvent.

Solute

The substance being dissolved in a solution.

Solvent

The dissolving medium in a solution, usually present in a greater amount.

Concentration

The amount of solute present in a given amount of solvent.

Saturated Solution

Contains the maximum amount of solute it can hold at a given temperature.

Unsaturated Solution

Contains less solute than it can hold at a given temperature.

Supersaturated Solution

Contains more solute than it can normally hold at a given temperature.

Nature of Solute and Solvent

"Like dissolves like"; polar solutes dissolve in polar solvents, and nonpolar solutes dissolve in nonpolar solvents.

Temperature

Affects solubility differently for gases and solids; solids generally become more soluble as temperature increases, while gases become less soluble.

Pressure

Affects the solubility of gases in liquids but has little effect on solids and liquids.

Surface Area

Smaller particles dissolve faster due to increased surface area.

Rate of Stirring

Increases solubility by allowing more contact between solute and solvent.

Reaction Stoichiometry

Describes quantitative relationships among substances in a chemical reaction.

Balanced Chemical Equation

Represents the number of moles of reactants and products in a reaction.

Mole Ratio

Ratio of the number of moles of reactants and products in a balanced equation.

Limiting Reactant

The reactant that is completely consumed first, limiting the amount of product formed.

Excess Reactant

The reactant that remains after the reaction is complete.

Theoretical Yield

Maximum amount of product that can be formed from given reactants.

Actual Yield

The measured amount of product obtained from a reaction.

Percent Yield

Ratio of actual yield to theoretical yield, expressed as a percentage.

Stoichiometric Coefficient

Numbers in a balanced equation representing the proportion of each substance.