Aircraft Maintenance Training Notes

Temperature measures the hotness or coldness of a substance. It influences the physical properties of fluids, especially when calculating gas state changes.

The centigrade scale uses the freezing and boiling points of water as its reference points, with 0°C for freezing and 100°C for boiling. It is divided into 100 equal divisions.

The Fahrenheit scale uses different reference points for freezing and boiling, with 32°F for freezing and 212°F for boiling.

The Kelvin scale uses absolute zero as its starting point, which is the theoretically lowest possible temperature. 0°K is equivalent to -273.15°C.

The amount of heat required to raise the temperature of a substance by one degree Celsius or one Kelvin. Higher heat capacity means greater resistance to temperature changes.

The amount of heat energy required to raise the temperature of one gram of a substance by one degree Celsius or one Kelvin. Specific heat is unique for each material.

The transfer of heat through direct contact between substances at different temperatures. Heat flows from the hotter object to the colder object.

The transfer of heat through the movement of fluids (liquids or gases). Hotter fluids rise, cooler fluids sink, creating a cycle of heat transfer.

The energy required to change the state of matter from a liquid to a gas, without altering the temperature.

The energy required to change the state of matter from a solid to a liquid, without altering the temperature.

The energy absorbed or released when the temperature of a substance changes. It causes changes in the temperature of the system.

The process of a liquid changing into a gas.

The temperature at which a liquid changes into a gas.

Heat transfer through the movement of fluids caused by differences in density, like hot air rising and cold air sinking.

Heat transfer through the direct movement of fluids by fans, pumps, or other devices, like a fan blowing air.

The process of heat transfer through electromagnetic waves, like the sun warming the Earth.

The amount of energy emitted by an object through radiation is directly proportional to the fourth power of its Kelvin temperature.

A type of convection where the fluid movement is driven naturally by differences in density created by temperature variations.

A type of convection where the fluid movement is forced by a fan, pump, or other device.

The transfer of energy through space via electromagnetic waves, like the sun's rays.

Thermal equilibrium is the state where the average kinetic energy of particles in two objects is equal. This means there's no net transfer of energy between them.

The particles inside a hot object have more kinetic energy than the particles in a cold object. This means the hot object's particles move faster.

In a collision between particles, energy is transferred. This means that collisions between particles are the mechanism for how objects reach thermal equilibrium.

When we average the effects of all collisions between particles in a sample of matter, we can understand how heat energy flows.

The perimeter of a sample of matter is the boundary where particles inside collide with particles of another substance.

At the perimeter of a sample of matter, particles collide with particles from a different substance. This is how energy is transferred between objects.

The kinetic energy of particles in a hot object decreases as energy is transferred to the cold object. The kinetic energy of particles in the cold object increases because it gains energy from the hot object.

The average kinetic energy of both objects becomes equal when they reach thermal equilibrium. This means both objects will have the same temperature.

The increase in volume of a solid per unit of its original volume for every degree Celsius rise in temperature.

A change in the length of a solid due to a change in temperature.

A change in the volume of a solid due to a change in temperature.

The change in volume (∆V) is directly proportional to the original volume (V) and the change in temperature (∆T).

The first law of thermodynamics states that energy cannot be created or destroyed, only transferred or transformed.

The internal energy of a system is the sum of the kinetic energy of its molecules and the potential energy stored in chemical bonds and intermolecular forces.

A system in thermodynamics can be any part of the universe you choose to study, separated from its surroundings.

The study of how heat and work affect the properties of a system, like temperature, pressure, and volume.

The process of a liquid turning into a gas, requiring energy input to overcome the forces holding the molecules together.

The process of a gas turning back into a liquid, releasing the energy that was absorbed during evaporation.

The energy absorbed or released during a phase change, such as evaporation or condensation.

The amount of heat energy needed to change a substance from a liquid to a gas at a constant temperature.

The amount of heat energy released when a substance changes from a gas to a liquid at a constant temperature.