E115_Problem_Set_17 - a = 1.36 ⋅ atm ⋅ mole –2 and b...

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e 115 Engineering Thermodynamics Fall 2009 University of California Problem set 17 Due: Wednesday, October 21 st , in discussion 1) (35 points) In lecture, we have been discussing the properties of a van der Waals gas. The equation of state for one mole of a van der Waals gas is given by: P + a V 2 V b ( ) = R T a) Develop an expression for c P c V for one mole of a van der Waals gas. (5 points) b) Develop expressions for the internal energy change, the enthalpy change, the entropy change, and the change in the Gibbs free energy when one mole of a van der Waals gas is isothermally expanded from an initial state P 1 , V 1 , T 1 ( ) to a final state P 2 , V 2 , T 2 ( ) . (8 points) c) Develop expressions for the work and heat when one mole of a van der Waals gas undergoes a reversible isothermal expansion. (5 points) d) Assuming that oxygen behaves as a van der Waals gas with
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Unformatted text preview: a = 1.36 ⋅ atm ⋅ mole –2 and b = 0.0318 ⋅ mole –1 , calculate the work, heat, internal energy change, enthalpy change, entropy change, and free energy change when one mole of oxygen gas is expanded from 1 to 2 at 300 K. Do the same calculations assuming that oxygen behaves as an ideal gas and compare your values. (12 points) e) Now consider that you would like to purchase oxygen for use in your lab. The oxygen gas will be stored at a pressure of 250 atm at room temperature in a cylinder that is 2 m high with a diameter of 0.25 m. If the vendor charges a price that is per liter of gas, would you prefer that the gas behaved ideally or as a van der Waals gas? (5 points)...
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