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CHEM 126 Chapter 6
CHEM 126 Final
| Question | Answer |
|---|---|
| heat | energy transferred between system & surroundings due to difference in temp (thermal) - thermal energy of molecule motion - Q |
| work | - energy transferred when object is moved by force - W |
| relationship between change in energy, heat, work | - ∆E = q + w |
| - Q > 0 - E increases | |
| heat FROM system TO surroundings | - q < 0 - E decreases |
| work done ON system BY surroundings | - w > 0 - E increases |
| work done BY system ON surroundings | - w < 0 - E decreases |
| E increases when.. | - Q > 0 - W > 0 |
| E decreases when... | - Q < 0 - W < 0 |
| P-V work | - W = -P * ∆V - use when rxn occurs that changes V of system - undergoes V change by pushing against surroundings -> do work |
| 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 |
| 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 |
| 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) |
| endothermic vs. exothermic | ∆H > 0: endothermic - absorb heat ∆H < 0: exothermic - release heat |
| 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 |
| constant pressure | - coffee cup calorimeter - qp = ∆H |
| constant volume | - bomb calorimeter - qv = ∆E (used for combustion) |
| 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) |
| 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 |
| 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 |
| hess's law + heat of formation | ∑(number of mols * heat of rxn(products)) - ∑(number of mols*heat of reaction(reactants)) |
Created by:
ccottrel
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