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HW 1.
Due: 9/30/11
NO CREDIT WILL BE GIVEN IF WORK IS NOT SHOWN!!
Problems (all from the textbook)
2.1 An ideal gas at 300 K has a volume of 15 liters at a pressure of 15 atm.
Calculate (1) the final volume of the system, (2) the work done by the system,
(3) the heat entering or leaving the system, (4) the change in the internal
energy, and (5) the change in the enthalpy when the gas undergoes
a. A reversible isothermal expansion to a pressure of 10 atm
b. A reversible adiabatic expansion to a pressure of 10 atm
(Assume monoatomic gas for this problem)
2.3 The initial state of a quantity of monoatomic ideal gas is P = 1 atm, V = 1 liter,
and T = 373 K. The gas is isothermally expanded to a volume of 2 liters and is
then cooled at constant pressure to the volume V. This volume is such that a
reversible adiabatic compression to a pressure of 1 atm returns the system to
its initial state. All of the changes of state are conducted reversibly. Calculate
the value of V and the total work done on or by the gas.
2.6 Ten moles of ideal gas, in the initial state P
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 Fall '11
 KIM

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