Suppose 1.0 mol of an ideal gas is initially at P=4.0 atm and T=400 K. It...

Suppose 1.0 mol of an ideal gas is initially at P=4.0 atm and T=400 K. It is expanded irreversibly and adiabatically against a constant pressure of 1.0 atm until the volume has doubled.
(a) Calculate the final volume of the gas.
(b) Calculate w, q, and energy change ΔU of this process, in joules.
(c) Calculate the final temperature of the gas.
(d) Calculate the entropy change ΔS of the ideal gas in the process.
(e) What is the entropy change of the surroundings, ΔS_surr, during this process? Does the results in (c) and (d) in combination satisfy the second law of thermodynamics? Explain

Expert Solution

genius_generous answered 1 year ago

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