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Chapter 6.3-6.4

CHEM 001A Chapter 6.3-6.4: Lecture 29 prereading.docx

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Arnold Yuan

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Lecture 29: Make it Work
6.3-6.4 pg. 234-246
(See Lecture 23 for 6.3)
6.4 Quantifying Heat and Work
heat – transfer of thermal energy
temperature – measure of thermal energy
thermal equilibrium – system and surroundings reach same temperature
q = CDT, where C is the heat capacity of the system: J/C
depending on system  higher heat capacity means smaller change in T for same amount
of heat
heat capacity – amount of heat required to change temperature by 1 C
- extensive property – depends on amount of matter
- intrinsic capacity – depends on type of matter
ospecific heat capacity (Cs) – amount of heat required to raise temperature
of 1 gram of substance by 1 C
intensive property – depend on kind of substance being heated,
not amount
oalso: molar heat capacity (J/mol C)
water has high heat capacity
q = m Cs DT
for closed system: qsys = -qsurr
pressure-volume work (alternative to heat as energy transfer is work (w))
w = FD
P = F/A
W = P A D
W = P A Dh (height of piston)
ADh = DV, if container is a cylinder
W = -PDV (negative because it’s on surroundings by system)
- interpretation: work caused by expansion of volume is negative of the pressure
that the volume expands against multiplied by the change in volume that occurs
during the expansion
- 101.3 J = 1 L atm
17.5 pg. 784-788
(see Lecture 27)
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