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work done by the system, is equal to the change in internal energy. Th e radiation (p. 98)
second law of thermodynamics states that heat fl ows from objects with second law of thermodynamics (p. 105)
a higher temperature to objects with a lower temperature. Entropy is a specifi c heat (p. 95)
thermodynamic measure of disorder; it is seen as continually increas- temperature (p. 88)
ing in the universe and may result in the maximum disorder called the
heat death of the universe.

APPLYING THE CONCEPTS

SUMMARY OF EQUATIONS 1. The Fahrenheit thermometer scale is
a. more accurate than the Celsius scale.
4.1 b. less accurate than the Celsius scale.
9 _
T F = T C + 32° c. sometimes more or less accurate, depending on the air
5 temperature.
d. no more accurate than the Celsius scale.
4.2
2. On the Celsius temperature scale
5 _
T C = (T F – 32°) a. zero means there is no temperature.
9
b. 80° is twice as hot as 40°.
4.3 c. the numbers relate to the boiling and freezing of water.
T K = T C + 273 d. there are more degrees than on the Fahrenheit scale.

4.4 Quantity of heat = (mass)(specific heat)(temperature change) 3. Internal energy refers to the
a. translational kinetic energy of gas molecules.
Q = mcΔT
b. total potential and kinetic energy of the molecules.
4.5 Heat absorbed or released = (mass)(latent heat of fusion) c. total vibrational, rotational, and translational kinetic energy
Q = mL f of molecules.
4.6 Heat absorbed or released = (mass)(latent heat of vaporization) d. average of all types of kinetic energy of the gas
molecules.
Q = mL v
4. External energy refers to the
4.7 (mechanical equivalence of heat)(quantity of heat) – (work) =
a. energy that changed the speed of an object.

internal energy difference between two states b. energy of all the molecules making up an object.
JQ – W = U 2 – U 1 c. total potential energy and kinetic energy of an object that

4.8 work =(mechanical equivalence of heat)(difference in heat you can measure directly.
d. energy from an extraterrestrial source.
input and heat output)
5. Heat is the
W = J(Q H – Q L )
a. total internal energy of an object.
b. average kinetic energy of molecules.
c. measure of potential energy of molecules.
d. same thing as a very high temperature.
6. The specific heat of copper is 0.093 cal/gC°, and the specific
KEY TERMS heat of aluminum is 0.22 cal/gC°. The same amount of energy
applied to equal masses, say, 50.0 g of copper and aluminum,
British thermal unit (p. 94) will result in
calorie (p. 94) a. a higher temperature for copper.
Celsius scale (p. 90) b. a higher temperature for aluminum.
conduction (p. 96) c. the same temperature for each metal.
convection (p. 97) d. unknown results.
entropy (p. 106) 7. The specific heat of water is 1.00 cal/gC°, and the specific heat of
external energy (p. 93) ice is 0.500 cal/gC°. The same amount of energy applied to equal
Fahrenheit scale (p. 90) masses, say, 50.0 g of water and ice, will result in (assume the ice
does not melt)

first law of thermodynamics (p. 104)
a. a greater temperature increase for the water.
heat (p. 93)
b. a greater temperature increase for the ice.
internal energy (p. 93)
c. the same temperature increase for each.
Kelvin scale (p. 91)
d. unknown results.
kilocalorie (p. 94)
8. The transfer of heat that takes place by the movement of groups
kinetic molecular theory (p. 86)
of molecules with higher kinetic energy is
latent heat of fusion (p. 100) a. conduction.
latent heat of vaporization (p. 100) b. convection.
molecule (p. 87) c. radiation.
phase change (p. 99) d. sublimation.
4-25 CHAPTER 4 Heat and Temperature 109