Thermodynamics and Gas Laws Lecture Review

Vocabulary flashcards covering key concepts from the lecture on thermodynamics and gas laws, including definitions for fundamental forces, ideal gas behavior, energy types, and the laws of thermodynamics.

Strong Force

One of the forces that attract atoms.

Electrostatic Force

One of the forces that attract atoms.

Boyle's Law

States that absolute pressure P and the volume V of a gas are inversely proportional, provided the temperature T and number of moles n are constant.

Charles's Law

A gas law where pressure P and number of moles n are constant, relating volume and temperature.

Gay-Lussac's Law

A gas law where volume V and number of moles n are constant, relating pressure and temperature.

Avogadro's Law

A gas law where pressure P and temperature T are constant, relating volume and number of moles.

Ideal Gas Equation

The equation PV = nRT, which describes the behavior of a perfect gas.

Concentration (Chemistry)

Expressed as moles of the volume (mols/volume).

Pressure

A force created by molecules bouncing around their container and pressing against the walls, defined as force over an area.

Compressibility Factor (z)

A 'fudge factor' used when the perfect gas equation no longer applies (e.g., for high-pressure gases), typically ranging from 0.2 to 0.4.

Van der Waals interactions

Weakest intermolecular forces, involving the attraction of electrons moving from one molecule to another.

Energy

The capacity to do work.

Work

Defined as a type of energy, calculated as force over distance (F*x) or pressure times change in volume (PΔV).

Potential Energy

Stored energy.

Kinetic Energy

Moving energy.

Internal Energy (U)

The connection of microscopic kinetic (translational, rotational, vibrational) and potential (vibrational, molecular) energies within a system.

Heat

Energy flow resulting from a temperature difference.

Reversibility

An idealized process in thermodynamics where energy transformations occur without friction and would oscillate forever.

Irreversibility

In reality, a process where friction converts macroscopic energy into microscopic energy, causing systems to eventually stop and warm the surroundings.

First Law of Thermodynamics

States that energy can neither be created nor destroyed, only transformed from one form to another, meaning it must be conserved.

Second Law of Thermodynamics

States that naturally occurring processes are directional and that entropy in a closed system either goes up with time or stays the same, imposing limits on how much heat can be converted to work.

Heat Engine

A device, such as a steam engine, internal combustion engine, or jet engine, that converts heat into work.

Heat Capacity (c)

The amount of heat (q) added per unit mass divided by the temperature change (ΔT).

Enthalpy (H)

The term ΔU + PΔV, which represents the total heat content of a system at constant pressure.