REPSIRATORY CARE UNIT II Lecture notes

Flashcards for Respiratory Care Unit II Lecture Notes focusing on key vocabulary terms related to energy, states of matter, gas laws, and related concepts.

Potential Energy

Energy of position; stored energy due to strong attractive forces between molecules, independent of the environment.

Kinetic Energy

Energy of motion; all matter possesses it, especially in gases due to weak attractive forces allowing free movement.

Solids

Maintain fixed shape and volume due to strong mutual attractive forces and close proximity of molecules; low kinetic energy.

Liquids

Molecules have less mutual attraction than solids, allowing more free movement but still relatively dense and not easily compressed.

Gasses

Have weak attractive forces, exhibit rapid, random motion, and frequent collisions; no fixed volume or shape, expanding to fill containers.

Viscosity

Thickness; opposition to flow in a liquid.

Cohesiveness

Unified; stick together as one body, referring to the cohesive properties of liquids.

Buoyant force

Forces of gravity around object have weak intermolecular forces

Density

Heavier substance particles that are packed more closely together in liquids.

Brownian motion

The random motion of smaller particles (suspended matter <3um) deposit in respiratory region of the lung where bulk gas flow cease and most aerosol particles reach the alveoli by depositing on surface walls and diffuse into the lungs.

Absolute Zero

A temperature at which all molecular activity ceases, representing a logical zero point for temperature scales. (-273, 0, -460)

Critical Temperature

The highest temperature at which a substance can exist as a liquid; above this temperature, a vapor cannot be liquefied regardless of pressure.

Critical Pressure

The lowest pressure necessary at the critical temperature of a substance to maintain it in a liquid state, maintaining equilibrium between liquid and gas forms.

Atmospheric Pressure

The force exerted on a surface by the air above it as gravity pulls it to the earth

Dalton’s Law (Partial Pressure)

The total pressure of a mixture of gases equals the sum of the partial pressures of all component gases.

Avogadro’s Law

Equal volume of gasses at same temperature and pressure must contain the same number of molecules.

Density

Ratio of a substance’s mass to volume.

Diffusion

The process whereby molecules move from an area of higher concentration to areas of lower concentration.

Graham’s Law (Gas Diffusion)

The rate of diffusion of a gas is inversely proportional to the square root of its gram molecular weight.

Henry’s Law

At a given temperature, the volume of a gas that dissolves in a liquid equals its solubility coefficient times its partial pressure.

Solubility Coefficient

The volume of a gas that will dissolve in 1ml of a given liquid at standard pressure and specified temperature.

Boyle’s Law

At constant temperature, the volume of a gas varies inversely with the pressure exerted on it.

Charles’ Law

If the pressure and the mass of a gas remain constant, the volume of the gas varies directly with the absolute temperature.

Gay Lussac’s Law

If the volume and mass of a gas remain constant, the pressure of the gas varies directly with the absolute temperature.