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11 Cards in this Set
- Front
- Back
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work
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-force x distance
-pressure volume work = (-Pext)(dV) |
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heat
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-q
-thermal energy transferred |
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first law of thermodynamics
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change in internal energy (dE) = q + w
= heat transferred + expansion work |
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equipartition theorem
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-energy of each degree of freedom of molecule at temp T is (1/2)kT
-determine heat capacities for ideal gases |
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internal energy of mole of monatomic molecules
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E = (3/2)nRT
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internal energy of mole of diatomic molecules
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E = (5/2)nRT
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internal energy of mole of nonlinear polyatomic molecules
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E = 3nRT
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H
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-enthalpy (state function)
- H = E + pV - enthalpy = heat for constant pressure |
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bond enthalpy
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enthalpy assos w/ dissoc of compound into fragments at standard state
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reversible isothermal expansion for ideal gas
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- dE = (Cv)(dT) **always true for ideal gas
- dT = 0, dE = 0, q = -w - w = -nRTln(V1/V2) |
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adiabatic expansion
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- q = 0, change in internal energy = work done
- pV^(gamma) = constant |
