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14 Cards in this Set
- Front
- Back
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1st law of thermodynamics |
Energy cannot be created or destroyed, only change forn |
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Equation for change in internal energy |
Change in energy = q + w Or: change in energy = q + (-P(change in volume)) |
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Constant pressure work conversion |
1 L*atm = 101.3 J |
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Specific heat capacity |
The amount of energy required to raise 1 g of a substance by 1 celsius or 1 kelvin |
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Constant-pressure calorimetry |
The system is open to the environment, allowing pressure to remain constant. Useful for reactions occurring in solution without gas formation, since any change in volume is negligible, and therefore the energy change can be measured directly as heat. |
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Constant-volume calorimetry |
Useful for reactions involving gases; since the volume is held constant, no work is performed, and therefore the change in energy can be measured solely via temperature change and the formula q = s*m*(change in T) |
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Change In energy equation |
(Change in energy) = nhv |
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Energy of a photon |
E = hv = hc/(wavelength) |
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De Broglie's equation |
Wavelength = h/mv |
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Bohr's model equation |
E = (-2.178*10^-18 J)(Z^2/n^2) (Z = nuclear charge) (Negative sign establishes that the electron has a lower energy closer to the nucleus as opposed to the reference point of the electron existing at an infinite distance.) Or: E = (-2.178*10^-18 J)(1/nfinal^2 - n0^2) |
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Pauli exclusion principle |
No two electrons in the same atom can have the same set of four quantum numbers. |
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State property |
A property dependent only on its present state. It does not matter when or how it got there, nor where it is going. Examples include elevation, energy change. |
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Extensive property |
A property depending directly on the amount of substance. |
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Intensive property |
A property that is independent of the amount of substance. |
