practice test 3-1

practice test 3-1 -...

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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:
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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 two-step 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. Answer 
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This note was uploaded on 12/06/2010 for the course CHEM 141 taught by Professor Freeman during the Spring '10 term at Columbia SC.

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practice test 3-1 -...

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