CHEM 126 Final
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| heat | energy transferred between system & surroundings due to difference in temp (thermal)
- thermal energy of molecule motion
- Q
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| work | - energy transferred when object is moved by force
- W
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| relationship between change in energy, heat, work | - ∆E = q + w
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| - Q > 0
- E increases
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| heat FROM system TO surroundings | - q < 0
- E decreases
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| work done ON system BY surroundings | - w > 0
- E increases
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| work done BY system ON surroundings | - w < 0
- E decreases
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| E increases when.. | - Q > 0
- W > 0
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| E decreases when... | - Q < 0
- W < 0
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| P-V work | - W = -P * ∆V
- use when rxn occurs that changes V of system
- undergoes V change by pushing against surroundings -> do work
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| units of energy | - E = (1/2)M*V^2
* mass = kg & volume = m/s
- 1 joule = 1 kg*m^2/s^2
- 1 caolire = 4.184 J
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| state function | - values depeond only on the state that the system is in, not path it took to get there
- EX: altitude, energy, enthalpy, pressure, volume, temp
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| change of enthalpy in terms of change of internal energy/heat | ∆E = q - P∆V
- at constant P (qp) = ∆E + P∆V
***** ∆H = ∆E + P∆V = qp
(P∆V is usually 0)
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| endothermic vs. exothermic | ∆H > 0: endothermic - absorb heat
∆H < 0: exothermic - release heat
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| specific heat capacity | - amount of heat required to change the temp of 1 gram of a material by 1 degree Kalvin
- Q = C * M * ∆T
- C = J/(g*K), M = grams, T = Kelvin, Q = Joules
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| constant pressure | - coffee cup calorimeter
- qp = ∆H
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| constant volume | - bomb calorimeter
- qv = ∆E (used for combustion)
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| constant pressure calometry equation | -T final water = T final solid
- q H20 = - q solid
- C H20 * M H20 * ∆T H20 = -(C solid * M solid * ∆T solid)
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| Hess's law | - ∆H rxn = sum of the enthalpy changes for the individual steps
** make sure excess elements cross off, moles match up, reverse sign if rxn needs to be reveresed
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| stand heats of rxn & standard heats of formation | - ∆H rxn° = ∆H rxn under standard conditions
- ∆H f° = enthalpy change for the formation of 1 mol of substance from its elements in their standard state
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| hess's law + heat of formation | ∑(number of mols * heat of rxn(products)) - ∑(number of mols*heat of reaction(reactants))
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