What is isothermal reversible expansion of an ideal gas?

In other words, in isothermal process ∆T = 0. Free expansion of a gas occurs when it is subjected to expansion in a vacuum (pex=0). During free expansion of an ideal gas, the work done is 0 be it a reversible or irreversible process. It is known that the change in internal energy of a system is given as: ∆U = q + w—(1)

What is reversible isothermal expansion?

Hence, a reversible isothermal expansion is an infinitely-slow increase in volume at constant temperature. For an ideal gas, whose internal energy U is only a function of temperature, we thus have for the first law of thermodynamics: ΔU=qrev+wrev=0.

What is reversible expansion of a gas?

The only way this is possible is if the pressure of the expanding gas is the same as the external pressure resisting the expansion at all points along the expansion. With no net force pushing the change in one direction or the other, the change is said to be reversible or to occur reversibly.

What is isothermal of real gases?

Thus, in an isothermal process the internal energy of an ideal gas is constant. This is a result of the fact that in an ideal gas there are no intermolecular forces. Note that this is true only for ideal gases; the internal energy depends on pressure as well as on temperature for liquids, solids, and real gases.

What is the difference between a reversible and irreversible gas expansion?

The difference is that one expansion is quasi-static (the reversible one) while the other is spontaneous because of a dramatic change of the external constraints (the irreversible one). In the quasi-static case, you start off indeed in the state where gas pressure equates external pressure.

What is the work done in isothermal reversible process?

Work done in an isothermal reversible expansion is maximum work. When the expansion of the gas is carried out reversibly then there will be series of such p. dV terms. The total maximum work Wmax can be obtained by integrating above equation between the limits V1 to V2.

Is reversible expansion of an ideal gas under isothermal condition?

Reversible expansion of an ideal gas under isothermal and adiabatic conditions are as shown in the figure. AB → Isothermal expansion. AC → Adiabatic expansion.

What is the difference between the work done between irreversible isothermal expansion and reversible isothermal expansion?

Work done in the isothermal reversible expansion of a gas is always greater than that done in isothermal irreversible expansion of the gas.

How can you show that work done in isothermal and reversible expansion of an ideal gas is the maximum?

In the reversible process, Pext is always less than the pressure of the gas, by an infinitesimally small quantity. In the equation W tends to the maximum as (P – dp) tends to P or dp tends to zero. Therefore work done in an isothermal reversible expansion of an ideal gas is maximum work.

Is work done in isothermal reversible expansion positive or negative?

Since the expansion is isothermal and of an ideal gas, the change in internal energy is zero. This means q = -w and for a compression, w is positive. Therefore q must be negative.

Which of the following are correct about irreversible isothermal expansion of ideal gas?

ΔT=0. Was this answer helpful?

What is the work done during the expansion of an ideal gas both in reversible and irreversible process?

Answer: During free expansion of an ideal gas, the work done is 0 be it a reversible or irreversible process. Where ∆U represents the change in internal energy, q is the heat given by the system and w is the work done on the system.

Why do reversible and irreversible expansion of gas differ in the work that they do on the surroundings?

The only way to transfer entropy to the surroundings is to transfer heat to the surroundings. This means more heat has to be transferred to the surroundings in an irreversible process than a reversible process. That leave less heat to be converted to work for the irreversible process than the reversible process.

What is the work done during the expansion of an ideal gas in reversible process?

zero
Solution : In both cases work done is zero because during free expansion of an ideal gas external pressure becomes zero.

What is the formula for isothermal irreversible expansion?

B. −wq=nRT[1−P2P1]

Why the work done in isothermal reversible expansion is more than that of irreversible expansion?

The reason why more work is done in a reversible process than an irreversible process is in an irreversible process entropy is generated within the gas whereas in a reversible process entropy is not generated.

Is an isothermal irreversible expansion of an ideal gas?

Assertion (A): ΔU=0 for a reversible as well as irreversible expansion of an ideal gas under isothermal conditions, whereas Stotal≠0 for an irreversible process. Reason (R) : ΔU=0 is independent of temperature whereas S is proportional to temperature.