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Winter 2011
Chemistry 163B
1
Homework #2
Problems (#6#15)
6.
E&R P2.6
AND
calculate q for each of the irreversible and reversible processes in parts a and b.
7.
One mole of ideal gas is heated reversibly at a constant pressure of 1 atm from
273.15 K to 373.15 K
a.
Compute the work involved in the process
b.
If the gas were expanded reversibly and isothermally at 273.15 K from an initial
pressure of 1 atm, what would the final pressure need to be in order to equal
the work calculated in part a?
8.
A
gas has the equation of state
! "
PV
RT
T P
#
$%
. For 1 mole of the gas:
a.
Show that for a reversible expansion between T
1
and T
2
at constant pressure
P, the work done is:
! " ! " ! "
! "
12
1
2
wRTT
T
T P
##
$&
%
&
b.
Show that for a reversible expansion between V
1
and V
2
at constant
temperature T, the work done is:
1
2
()
ln
'(
&
$
±*
&
+²
VT
wR
T
9.
One mole of ideal gas at 298 K is in a piston at a pressure of 100 atm.
a.
What is the work done by the gas if it expands isothermally against a constant
pressure of 10 atm?
b.
What is the total work done by the gas if the piston expands against constant
pressure in 3 stages, reaching equilibrium between each stage:
first against 50 atm, then against 20 atm, and finally against 10 atm.
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This note was uploaded on 03/16/2011 for the course CHEM 163B taught by Professor Geneswitkes during the Spring '11 term at University of California, Santa Cruz.
 Spring '11
 GeneSwitkes
 Mole

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