What is the free expansion of an ideal gas under adiabatic condition?

For an adiabatic process, q = 0 and for free expansion, W = 0, Therefore ΔT = 0.

Is an isothermal process also adiabatic?

Yes, an isothermal process can be adiabatic. It can happen in irreversible processes. Examples include free expansion[1] and Joule-Thompson expansion of an ideal gas.

Is the isothermal expansion of an ideal gas spontaneous?

During this constant temperature, or isothermal, expansion into a vacuum, the gas does no work (w = 0) and no heat is transferred between the system and surroundings (q = 0). Thus, E = 0 for the expansion. Nevertheless, the process is spontaneous.

What is free expansion of an ideal gas?

The free expansion of a gas is a process in which a gas is allowed to expand into the vacuum. Thus, the change in the internal energy of the ideal gas in free expansion is zero. As the change in the internal energy of an ideal gas in the free expansion is zero. Thus, option (A) remains constant is correct.

What is meant by free expansion of an ideal gas?

The Joule expansion (also called free expansion) is an irreversible process in thermodynamics in which a volume of gas is kept in one side of a thermally isolated container (via a small partition), with the other side of the container being evacuated.

Which of the following is correct for free expansion of an ideal gas under?

For the free expansion of an ideal gas, the opposing force is zero, hence work done = 0.

Can a process on ideal gas be both adiabatic and isothermal?

if the process is adiabatic as well as isothermal, no work will be done. So, a process on an ideal gas cannot be both adiabatic and isothermal.

What is isothermal and adiabatic expansion?

The word ‘isothermal’ means constant temperature. An isothermal process is a process occurring at a constant temperature. The word ‘adiabatic’ means isolated from surroundings. Adiabatic process means a process that neither allows the heat to transfer inside nor let the heat out of the system.

What is isothermal expansion in the context of an ideal gas?

Isothermal Expansion This shows the expansion of gas at constant temperature against weight of an object’s mass (m) on the piston. Temperature is held constant, therefore the change in energy is zero (U=0). So, the heat absorbed by the gas equals the work done by the ideal gas on its surroundings.

What is correct about isothermal expansion of the ideal gas?

Thus, in an isothermal process the internal energy of an ideal gas is constant. If the gas is ideal, the amount of energy entering the environment is equal to the work done on the gas, because internal energy does not change. For isothermal expansion, the energy supplied to the system does work on the surroundings.