In an isothermal process, the internal energy of an ideal gas remains constant.

In adiabatic compression, the temperature of a gas increases due to work done on it.

During a phase change, the temperature of a substance remains constant despite heat being added or removed.

In an isothermal process, the temperature of the system remains constant.

Conduction occurs when heat is transferred through direct contact, such as heating water in a pot.

In isothermal expansion, a gas does work on its surroundings as it expands.

Convection is the process of heat transfer that occurs due to the movement of fluid, where warmer areas of a liquid or gas rise and cooler areas sink.

Conduction is the process where heat is transferred through a material without any movement of the material itself.

A hot cup of coffee cooling down involves conduction (heat transfer from coffee to cup) and convection (heat transfer from cup to air).

The heat transfer coefficient in convection depends on surface area, fluid velocity, and temperature difference.

Fourier's Law of Heat Conduction states that the rate of heat transfer by conduction is directly proportional to the area and the temperature gradient.

The rate of heat transfer by conduction is directly proportional to the temperature difference between the two ends.

The Stefan-Boltzmann Law relates to radiation, stating that the total energy radiated per unit surface area is proportional to the fourth power of the black body's temperature.

The first law of thermodynamics states that the total energy of an isolated system is constant, meaning energy can neither be created nor destroyed.

During a reversible isothermal expansion, the entropy of the system increases as the gas expands and does work on the surroundings.

In a reversible process, the total entropy of the system and surroundings remains constant.

In a spontaneous process, the entropy of a system increases.

The second law of thermodynamics states that the entropy of an isolated system always increases.

In free expansion, no work is done and no heat is exchanged, so the internal energy remains constant.

In an isochoric process, the volume remains constant, and any heat added to the system increases the internal energy of the gas.

In an adiabatic compression, work is done on the gas, which increases its internal energy.

According to Boyle's law, for a given amount of gas at constant temperature, pressure is inversely proportional to volume. Halving the volume doubles the pressure.

The rate of heat transfer decreases with an increase in thickness, as per Fourier's Law.

During adiabatic expansion, a gas does work on its surroundings, which results in a decrease in temperature.

During a phase change, the temperature of a substance remains constant while heat is added or removed.

During a phase change, the thermal energy remains constant as the energy is used to change the state rather than increase the temperature.

In an isochoric process, the change in internal energy is equal to the heat added to the system, ΔU = Q.

In an isochoric process, the change in internal energy is equal to the heat added to the system, ΔU = Q.

In an isochoric process, the volume remains constant, and the change in internal energy is equal to the heat added to the system.

In an isochoric process, the volume remains constant, and any heat added to the system increases the internal energy of the gas.