Thermodynamics primarily focuses on energy transfer in various systems.

The First Law of Thermodynamics is the law of energy conservation.

Entropy is a measure of the disorder or randomness in a system.

This equation represents the First Law of Thermodynamics, where ΔU is the change in internal energy, Q is heat, and W is work.

Adiabatic processes involve no heat exchange with the surroundings.

Gibbs Free Energy is the thermodynamic function that represents the maximum useful work.

The relationship between entropy change, heat transfer, and temperature is ΔS = Q/T.

Standard state conditions are generally defined as 1 atm pressure and 25°C for thermodynamic calculations.

The Joule-Thomson effect describes the temperature change during an isenthalpic process.

The Third Law of Thermodynamics states that as a system approaches absolute zero, the entropy approaches a minimum constant value.

The Clausius statement of the Second Law is related to the increase in entropy in natural processes.

The standard enthalpy of formation for an element in its most stable form is defined as 0 kJ/mol.

An endothermic process absorbs heat from the surroundings.

The Carnot cycle is an idealized cycle for a heat engine.

At equilibrium, the standard Gibbs free energy change (ΔG°) for a reaction is 0 kJ/mol.

Enthalpy is most relevant to processes that occur at constant pressure.

The Maxwell-Boltzmann distribution describes the distribution of molecular velocities in a gas.

The standard entropy change for a pure crystalline substance at absolute zero is 0 J/(mol·K).

In a spontaneous process, the change in Gibbs free energy (ΔG) is negative.

The First Law of Thermodynamics is also known as the law of conservation of energy.

The heat capacity at constant volume (Cv) is defined as the change in temperature.

An isothermal process occurs when the temperature remains constant.

The relationship is ΔG° = -RT ln(K), where R is the gas constant and T is the absolute temperature.

The term "enthalpy" is often represented by the symbol H in thermodynamic equations.

The standard enthalpy change (ΔH°) for a reaction carried out under standard conditions is defined as 0 kJ/mol.

The van't Hoff equation relates the change in equilibrium constant with temperature.

The term "adiabatic" comes from the Greek words meaning "without heat exchange."

Chemical thermodynamics primarily focuses on heat transfer in chemical reactions.

The Stefan-Boltzmann Law describes the relationship between temperature and radiant energy emission.

In thermodynamics, the term "work" is typically represented by the symbol W.

The relationship is ΔG° = -RT ln(K), where R is the gas constant and T is the absolute temperature.

Exothermic processes release heat to the surroundings.

In a reversible process, there is no net change in entropy for the universe.

Internal energy is the sum of kinetic and potential energy of the system.

Boyle's Law describes the relationship between pressure and volume, keeping temperature constant.

The term "enthalpy of reaction" (ΔHrxn) is also known as the heat of reaction.

The relationship is Q = mcΔT, where Q is heat transfer, m is mass, c is specific heat, and ΔT is temperature change.

According to the Second Law, the entropy of the universe tends to increase.

The Gibbs-Helmholtz equation relates the change in Gibbs free energy (ΔG) with temperature.

Joule's Law describes the relationship between the internal energy change (ΔU) and temperature.

The process of phase transition from gas to liquid is called condensation.

The Antoine equation is used to describe the vapor pressure of a substance.

The heat capacity at constant pressure (Cp) for an ideal monatomic gas is (5/2)R.

The standard entropy of a substance is defined at 1 atm pressure and 25°C.

The heat capacity ratio (γ) for a diatomic ideal gas is approximately 1.4.

Kirchhoff's Law relates the change in enthalpy (ΔH) with temperature and pressure.

The slope of the P-V diagram for an adiabatic process is equal to the heat capacity ratio (γ).

An isobaric process is a process with constant pressure.

The Carnot efficiency is given by 1 - T₂/T₁ for a heat engine operating between two temperatures T₁ and T₂.

The Nernst equation relates the standard cell potential (E°cell) with the concentration of ions in a cell.

The triple point of water is defined at 0°C and 0 K.

The Clausius-Clapeyron equation describes the relationship between vapor pressure and temperature.

The R value in the ideal gas law equation represents the gas constant.

Enthalpy of combustion is related to the heat transfer during combustion reactions.

The van der Waals equation corrects the ideal gas law for molecular interactions.

An adiabatic wall is a boundary that allows no heat transfer.

The relationship is ΔH = ΔU + PΔV, where ΔH is enthalpy change, ΔU is internal energy change, P is pressure, and ΔV is volume change.

The standard molar entropy (S°) for a substance is measured in units of J/(mol·K).

In thermodynamics, work is considered positive when the surroundings do work on the system.

The critical point of a substance is the point at which it becomes a supercritical fluid.

The P-T diagram for a phase transition is represented by a line with a negative slope for condensation.

An adiabatic wall is a boundary that allows no heat transfer.

The heat capacity at constant volume (Cv) is equal to the change in internal energy.

A reversible process can be brought back to its initial state with no change in entropy for the universe.

The heat capacity ratio (γ) is also known as the adiabatic index or isentropic exponent.