Is isothermal expansion of ideal gas reversible?

During free expansion of an ideal gas, the work done is 0 be it a reversible or irreversible process. Isothermal reversible change: q = -w = pex(Vf-Vi) Isothermal reversible change: q = -w = nRTln (Vf/Vi) = 2.303 nRT log (Vf/Vi) Adiabatic change: q =0, ∆U = w.

What is enthalpy change in isothermal reversible expansion?

Isothermal Expansion 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. Enthalpy change is also equal to zero because the change in energy zero and the pressure and volume is constant.

What is correct about isothermal expansion of the ideal gas?

Hint: The isothermal expansion means a gas is expanding from initial volume to final volume at constant temperature. So, during the isothermal expansion of an ideal gas, the temperature remains constant and volume increases. Internal energy is a function of temperature and volume.

Why is isothermal expansion reversible?

A process that takes place with zero entropy change is reversible because energy has not been “degraded.” In a reversible isothermal expansion, you have both reversible work and reversible heat transfer.

How does entropy change in a reversible isothermal expansion?

Homework Help: Entropy change in a reversible isothermal process. 1. In a reversible isothermal expansion of an ideal gas, as the gas expands, heat is supplied to it, so that the temperature remains constant.

What is the ΔH of the reversible expansion of ideal gas?

Since its isothermal, δ U is zero. But enthalpy change δ H is δ U + δ n ( gaseous) R T or δ H = δ U + δ ( p V). For reversible isothermal expansion of ideal gas, what is the δ H, is it positive, negative or zero.

Why is ΔU 0 for an isothermal reversible process?

It should be noted (although it will be proven in a later chapter) that ΔU for an isothermal reversible process involving only p-V work is 0 for an ideal gas. This is true because the internal energy, U, is a measure of a system’s capacity to convert energy into work. In order to do this, the system must somehow store that energy.

How does isothermal expansion work in the environment?

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. In either case, with the aid of a suitable linkage the change in gas volume can perform useful mechanical work.