General Chemistry II Practice Flashcards (Lectures 24-33)

A set of 10 vocabulary flashcards covering key concepts from General Chemistry II lectures regarding thermodynamics, electrochemistry, and nuclear chemistry.

Spontaneous Process

A process that occurs without outside intervention, which can proceed regardless of the speed or rate of the reaction.

Entropy ($S$)

A measure of the disorder of a system, statistically defined by the equation $S = k\,\ln(W)$ where $k$ is the Boltzmann constant ($1.38 \times 10^{-23}\,J/K$) and $W$ is the number of microstates.

First Law of Thermodynamics

The principle stating that the energy of the universe is constant, although various forms of energy can be interchanged during physical and chemical processes.

Second Law of Thermodynamics

The law stating that in any spontaneous process, there is always an increase in the entropy of the universe.

Third Law of Thermodynamics

The law stating that a perfect crystal at absolute zero ($0\,Kelvin$) has an entropy value of zero.

Gibbs Free Energy ($G$)

The maximum amount of non-expansion work that can be extracted from a closed system, where a negative change (\Delta G < 0) indicates a spontaneous process.

Electrochemistry

The study of the interchange between chemical change and electrical work, involving systems like electrochemical cells to produce or use electrical energy.

Faraday's Constant ($F$)

A constant representing the magnitude of electric charge per mole of electrons, given as $96,485\,C/mol$.

Mass Defect

The difference between the actual mass of a nucleus and the theoretical sum of the masses of its constituent protons and neutrons.

Nuclear Binding Energy

The energy released when a nucleus is formed from its constituent particles, calculated using Einstein's equation $E = mc^2$.