Chemical Thermodynamics and the 1st Law of Thermodynamics

Flashcards covering key concepts, terms, and laws of chemical thermodynamics from the lecture notes.

Thermodynamics

The study of the movement of thermal energy within a system.

Chemical Thermodynamics

Studies the interrelation of heat and work with chemical reactions or with physical states according to the laws of thermodynamics.

Heat (q)

Transfer of thermal energy, represented in Joules (J).

Work (w)

Force used to transfer energy between a system and its surroundings, also represented in Joules (J).

System

Any part of the universe that we choose to study.

Surroundings

Everything outside the system.

Universe

The entirety of the system and its surroundings.

Zeroeth Law of Thermodynamics

If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other.

First Law of Thermodynamics

The energy of the universe is constant; energy can be transformed but not created or destroyed.

Second Law of Thermodynamics

Entropy of the universe increases in spontaneous processes and remains unchanged in equilibrium processes.

Third Law of Thermodynamics

At absolute zero, the entropy of a perfect crystal is zero.

Exothermic Reaction

A process that releases heat, such as combustion of fuels.

Endothermic Reaction

A process that absorbs heat, such as melting of ice.

Entropy

A measure of disorder in a system, representing energy unavailable to do work.

Gibbs Free Energy (G)

Energy available to do work in a system, represented by the equation G = H - TS.

Spontaneous Process

A process that occurs without the need for external energy.

Non-Spontaneous Process

A process that requires outside intervention or energy to occur.

Standard Entropy Change (∆S°)

Calculated as the difference in standard entropy between products and reactants during a reaction.