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Two moles of an ideal gas are allowed to expand reversibly and isothermally at 300 K from a
pressure of 1 atm to a pressure of 0.1 atm. What is the change in Gibbs free energy?�

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Related questions

If 2.0 mol of an ideal gas, initially at 1.53 atm and 280 K, is allowed to expand isothermally under a constant external pressure of 0.92 atm until the final internal pressure is 0.92 atm, what is the work done ?

3. (Castellan, Problem 9.18) Consider one mole of an ideal gas, CV = 3/2R, the initial state: 300K, 1atm. For each transformation, (a) through (g), calculate Q, W, ∆E, ∆H, and ∆S; compare ∆S to Q/T.

a) At constant volume, the gas is heated to 400K.

b) at constant pressure, 1 atm, the gas is heated to 400K.

c) The gas is expanded isothermally and reversibly until the pressure drops to 1/2 atm.

d) The gas is expanded isothermally against a constant external pressure equal to 1/2 atm until the gas pressure reaches 1/2 atm.

e) The gas is expanded isothermally against zero opposing pressure (Joule expansion) until the pressure of the gas is 1/2 atm.

f) The gas is expanded adiabatically against a constant pressure of 1/2 atm until the final pres- sure is 1/2 atm.

g) The gas is expanded adiabatically and reversibly until the final pressure is 1/2 atm.

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