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.

Increasing the surface area of an object increases the rate of heat transfer, as more area is available for heat exchange.

Increasing the surface area of an object increases the rate of heat transfer by radiation, as more surface is available for emitting energy.

Increasing the temperature of a gas at constant volume results in an increase in pressure, according to Gay-Lussac's law.

The efficiency of a Carnot engine is given by the formula: efficiency = 1 - (T2 / T1), where T1 is the higher temperature and T2 is the lower temperature.

The entropy change for a reversible isothermal expansion of an ideal gas is ΔS = nR ln(Vf/Vi).

The entropy change for a reversible isothermal process is ΔS = nR ln(Vf/Vi).

For a reversible process, the entropy change can be zero if the process is isothermal and reversible.

Using the formula m1*T1 + m2*T2 = (m1 + m2)*Tf, we find Tf = (200*90 + 300*30) / (200 + 300) = 70°C.

The first law of thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another.

Q = m*c*ΔT = 250 g * 0.9 J/g°C * (75°C - 25°C) = 4500 J.

The latent heat of fusion for ice is approximately 334 J/g.

Latent heat of fusion is the heat required to change a solid into a liquid at its melting point.

Convection is the primary mechanism of heat transfer in liquids and gases due to the movement of the fluid.

In liquids, convection is the main mechanism of heat transfer, as the fluid moves and carries heat with it.

Convection is the mode of heat transfer that occurs through a fluid due to density differences.

Conduction is the mode of heat transfer that occurs through a solid or stationary fluid without any movement of the fluid itself.

All of the above factors affect the rate of heat transfer by conduction.

In a vacuum, heat transfer occurs primarily through radiation, as there are no particles to conduct or convect heat.

In liquids and gases, convection is the primary mechanism of heat transfer, as it involves the movement of fluid.

In liquids, convection is the primary mechanism of heat transfer, although conduction and radiation can also occur.