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Unformatted text preview: Calculate the work done by decreasing the pressure of a 7.3 mol He at 77°C reversibly from 2.0 atm to 1.0 atm. Assume that Helium behaves as an ideal gas. Give your answer (including sign) in kJ to 3 significant figures. Answer 2. Calculate the heat that must be supplied to a 75.0 gram glass vessel containing 1.5 L of water to raise its temperature from 25.0°C to 37.0°C. Give your answer in kJ to 3 significant figures. C s (H 2 O) = 4.18 J ∙ (°C) − 1 ∙ g − 1 C s (glass) = 0.78 J ∙ (°C) − 1 ∙ g − 1 Answer 1.00 mol of an ideal gas undergoes the reversible pathway shown in the diagram below: 3. The work done from B to C is: A. w = +864 J B. w = 1441 J C. w = 0 D. w = −864 J 4. The work done from C to D is: A. w = 0 B. w = −864 J C. w = +864 J D. w = − 1441 J 5. Calculate the change in the internal energy of the gas for the whole process. Answer 6. A system undergoes a twostep process. In step 1, it expands adiabatically from 1.00 L to 2.56 L at 1.00 atm. In step 2, it releases 73 J of heat at 1.00 atm as it returns to the original internal energy. Find the final volume of the system. Give your answer in L to two significant figures....
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 Fall '08
 FREEMAN
 Thermodynamics, Enthalpy, Entropy

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