Thermodynamics and Thermochemistry Overview

These flashcards cover essential vocabulary and key concepts related to thermodynamics and thermochemistry, including definitions of terms and principles discussed in the lecture notes.

First Law of Thermodynamics

Energy cannot be created or destroyed, only transformed from one form to another.

System

The specific portion of matter under study, separated from its surroundings by a boundary.

ΔU

Change in internal energy, calculated as ΔU = q + w, where q is heat and w is work.

Isothermal Process

A process that occurs at a constant temperature.

Kinetic Energy (EK)

The energy of a particle due to its motion, calculated as EK = ½ mv².

Thermochemistry

The study of the heat energy associated with chemical reactions.

Exothermic Reaction

A chemical reaction that releases heat to the surroundings.

Endothermic Reaction

A chemical reaction that absorbs heat from the surroundings.

Heat Capacity (C)

The quantity of heat needed to raise the temperature of a substance by one degree Celsius.

Specific Heat Capacity (s)

The heat required to raise the temperature of one gram of a substance by one degree Celsius.

Molar Heat Capacity

The heat capacity for one mole of a substance.

Calorimeter

A device used to measure the heat absorbed or evolved during a physical or chemical change.

Intensive State Variable

A property that does not depend on the size of the system, such as temperature or pressure.

Extensive State Variable

A property that depends on the size of the system, such as mass or volume.

Enthalpy (H)

A thermodynamic potential that measures the total heat content of a system.