CHEM 2P03 Test 1
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40 Terms
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0th Law of Thermodynamics
if two thermodynamic systems each are in thermal equilibrium with a third, then they are in thermal equilibrium with each other
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temperature
a property that determines the direction of heat flow when an object is in contact with another object
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internal energy (U)
kinetic energy + potential energy
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ideal gases
have no interactions between particles; the internal energy is only a function of temperature and not a function of pressure or volume
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variables of state
depend on the state of the system and not how the system arrived at that state
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variables of state examples
pressure, volume, temperature, internal energy
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work (w)
ordered kinetic energy, no entropy component, high quality
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heat (q)
disordered kinetic energy, entropy component, low quality
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transfer of internal energy
delta U = q + w
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exothermic process
q < 0; heat leaves the system
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endothermic process
q > 0; heat enters the system
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1st Law of Thermodynamics
energy is conserved; the total energy of the system and the surroundings is constant
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isothermal
constant temperature (delta T = 0)
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isochoric
constant volume (deltaV = 0, w = 0)
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isobaric
constant pressure (deltaP = 0)
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adiabatic
no heat is transferred (q = 0)
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cyclic
no change in state variables (final state = initial state)
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intensive variables of state
independent of the amount of material (eg. pressure, temperature, specific and molar heat capacity, density)
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extensive variables of state
proportional to the amount of material (eg. volume, mass, internal energy, entropy, heat capacity)
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isothermal expansion of ideal gases
qT OR wT
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Cv
heat capacity at a constant volume
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Cv of a monoatomic gas
3/2R
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Cv of a diatomic gas (small)
5/2R
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Cv of a diatomic gas (large)
7/2R
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Cv of a linear polyatomic gas
5/2R
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Cv of a non-linear polyatomic gas
3R
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isobaric expansion of ideal gases
qP OR wP
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liquid/solid energy and enthalpy
deltaU approx. equal to deltaH; Cp
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standard enthalpy per mole
the enthalpy of formation of 1 mol of the compound at 1 bar pressure from its elements in their standard states
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adiabatic reversible expansion
use Cvln(T2/T1) = -Rln(V2/V1)
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real gas law A term
accounts for attractive forces between molecules
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real gas law B term
accounts for the intrinsic volume of gas molecules
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Joule-Thomson Experiment
measuring the temperature of a gas (T1, T2) before and after it expands from P1 to P2 through a porous plug
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Joule-Thomson coefficient for ideal gases
0
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Joule-Thomson coefficient for real gases
depends on changes in internal energy during expansion caused by intermolecular interactions
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Carnot Cycle 1 to 2
isothermal reversible expansion; top left-right curve
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Carnot Cycle 2 to 3
adiabatic reversible expansion; right up-down curve
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Carnot Cycle 3 to 4
isothermal reversible compression; bottom right-left curve
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Carnot Cycle 4 to 1
adiabatic reversible compression; left down-up curve
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efficiency
1 - (Tcold/Thot)
Note 
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