(Serway, Faughn, Vuille, and Bennett, chapters 10− 12)
1.
An automobile fuel tank is filled to the brim with 45 L (12 gal) of gasoline at 10 °C. Immediately
afterward, the vehicle is parked in the sunlight, where the temperature is 35 °C. How much gasoline
overflows from the tank as the result of the expansion? (Neglect the expansion of the tank.) The
4
1
average coefficient of volume expansion for gasoline is 9.6x10− °C− .
(10)
2.
An iron ball of mass 500 g at a temperature of 500 °C is cooled by placing it on a block of ice taken
from the freezer. If the mass of the ice is 800 g and its initial temperature is −10 °C, then what is the
final configuration? That is, is the final state of the H2O all ice, ice-water mixture, water only, watersteam mixture, or steam only? If it is a mixture, determine the proportions. Find the final temperature.
The specific heat of iron is 0.107 cal/g•°C.
Hint: determine the energy required for the H2O to bring it to each end of a phase transition, and
calculate the energy available from the iron for each of these points.
(25)
3.
Complete the following table:
ΔU
isobaric
nCVΔT
(20)
Q
W
_______________
________________
isovolumetric
_______________
_______________
________________
isothermal
_______________
_______________
−nRT ln(Vf/Vi)
adiabatic
_______________
_______________
________________
4.
State the four laws of thermodynamics.
5.
Using the standard container of an ideal gas in a cylinder with a movable piston on the top, explain
why CV is different from CP. Which is larger and why?
(10)
6.
Thermal energy may be transferred from one place to another. What are these mechanisms?
Describe each briefly and discuss the type of material that each might take place (solid, liquid, gas, or
vacuum).
(15)
23
NA = 6.02x10 particles/mole
23
kB = 1.38x10− J/K
1 calorie
H2O:
=
4.186 J
cice = 0.500 cal/g•°C
heat of fusion = 79.7 cal/g
(20)
R = 8.31 J/mole•K
absolute zero = −273.15°C
cwater = 1.000 cal/g•°C
csteam = 0.480 cal/g•°C
heat of vaporization = 540 cal/g