One mole of an ideal monatomic gas initially at 300 K and a pressure of 15.0...

One mole of an ideal monatomic gas initially at 300 K and a pressure of 15.0 atm expands to a final pressure of 1.00 atm. The expansion can occur via any one of four different paths: a. isothermal and reversible, b. isothermal and irreversible, c. adiabatic and reversible, and d. adiabatic and irreversible. In irreversible processes, the expansion occurs against an external pressure of 1.00 atm. For each case, calculate the values of q, w, DU, and DH. I need the most help with C. and D.

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queen_honey_blossom answered 2 years ago

25 pts) One mole of ideal, monatomic gas, initially at T = 250 K and pressure...

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One mole of an ideal monatomic gas is expanded from an initial state at 3 bar and 450 K to a final state at 2 bar and 250 K. There are two different paths for this expansion: path 1: (1 mole ideal gas, 3 bar, 450 K) → (1 mole ideal gas, 3 bar, 250 K) → (1 mole ideal gas, 2 bar, 250 K) path 2: (1 mole ideal gas, 3 bar, 450 K) → (1 mole ideal gas,...

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5 moles of ideal gas is initially at 300 K and 5 bar. It is compressed to 10 bar at 300 K. This change is carried out by two different reversible processes: A: heating at constant volume followed by cooling at constant pressure B: cooling at constant pressure followed by heating at constant volume Depict these processes on a PT graph. (Hand drawn on engineering sheet would suffice). Calculate ΔU, ΔH, Q, and W requirements for each path. Cv=20.78 J/mol.K...

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