Ideal Gases and Thermodynamics Concepts

At constant volume, the pressure of a gas is directly proportional to its absolute temperature.

PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the universal gas constant, and T is temperature.

PV = NkT, where P is pressure, V is volume, N is the number of molecules, k is Boltzmann's constant, and T is temperature.

An idealized model of a real gas where molecules have negligible volume and attraction, and collisions are perfectly elastic.

A model describing the behavior of gas molecules based on their motion, collisions, and interactions.

6.022 x 10^23, representing the number of molecules in one mole of a substance.

A fundamental constant relating the average kinetic energy of gas molecules to their temperature: 1.38 x 10^-23 J/K.

A theoretical gas composed of many randomly moving point particles that do not interact, except during elastic collisions. These collisions do not dissipate energy, and there are no attractive or repulsive forces between the particles.

At a constant temperature, the pressure and volume of a fixed amount of gas are inversely proportional.

At constant pressure, the volume of a fixed amount of gas is directly proportional to temperature (in Kelvin).

At constant volume, the pressure of a fixed amount of gas is directly proportional to temperature (in Kelvin).

Any change in the state of a thermodynamic system or the changes it undergoes during a period of time.

A thermodynamic process that occurs at constant volume.

A thermodynamic process that occurs at constant pressure.

A thermodynamic process that occurs at constant temperature.

A thermodynamic process with no heat exchange.

A thermodynamic process where the system returns to its initial state after a series of changes.

Energy cannot be created or destroyed; it can only be transferred or changed from one form to another.

A graph showing the pressure-volume relationship of a thermodynamic system.

Calculated using the formula dW = PdV, where P is the pressure and dV is the change in volume.

The quantity of a substance containing the same number of particles as 12 grams of carbon-12, which is approximately 6.022 x 10^23 particles.

The number of particles (atoms, molecules, etc.) in one mole of a substance, approximately 6.022 x 10^23.

The study of energy transfer and transformations in a system, considering heat, work, and temperature.

The specific collection of objects in a thermodynamic study, focusing on specific processes within the group of objects.

The environment outside the thermodynamic system.

The dividing line between the system and its surroundings.

A thermodynamic system where both energy and matter can be transferred between the system and its surroundings.

A thermodynamic system where only energy can be transferred between the system and its surroundings.

A thermodynamic system where neither energy nor matter can be transferred between the system and its surroundings.

The total kinetic and potential energy of all the molecules within a system.

Energy transfer due to a temperature difference between a system and its surroundings.

Energy transferred when a force causes displacement.

Energy associated with the motion of particles in a system.

Energy associated with the arrangement or position of matter, like chemical bonds.

A restatement of the law of conservation of energy for thermodynamic systems. It states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.

Describes systems in thermal equilibrium.

Systems that have reached thermal equilibrium are at the same temperature and will not exchange thermal energy.

The total energy of a thermodynamic system.

The transfer of thermal energy.

Energy transferred to or from a system by applying a force.

Heat (Q) is positive when added to system, negative when removed. Work (W) is positive when done on the system, negative when done by the system.

A device that converts internal energy into more useful forms, such as mechanical or electrical energy.

Three essential features to operate a heat engine: 1. Heat input at a high temperature; 2. Part of the heat used for work; 3. Remainder of heat rejected at a lower temperature.

A measure of the proportion of input heat converted to work.

Achieved when all heat input is converted to work, i.e. no heat is lost to a cold reservoir.

A process where both the system and its surroundings can return to their original states after the process.

An ideal heat engine that operates in a reversible cycle between two reservoirs.

Any real heat engine operating between two temperature reservoirs will always have a lower efficiency than a Carnot engine operating between the same reservoirs.

The efficiency of a Carnot engine, which depends on the temperature of the high and low temperature reservoirs.

The temperature scale to use for calculating the efficiency of a Carnot engine.

All Carnot engines, working between the same hot and cold reservoirs, have the same efficiency.

Carnot engine efficiency is 100% (1.0) if the cold reservoir temperature is 0 Kelvin.

Carnot engines are the most efficient because their processes are reversible.

Processes like friction reduce engine efficiency because they lower heat-to-work conversion.

A property of a system that measures its disorder (or randomness).

Entropy is a function of the system's state, like internal energy.

A system exhibiting high order (organization).

A system exhibiting high disorder (randomness).

Melting of ice, or shattering of glass, shows an increase of disorder and increase in entropy of the system.

Change in entropy calculated as heat transferred (Q) divided by temperature (T) = ΔS = Q/T