Chemistry 120 Test 2 Ellis
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| Kinetic Molecular Theory #1 | The volume of individual particles of a gas can be assumed to be negligible.
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| Kinetic Molecular Theory #2 | The particles are in constant motion, the collision of the particles creates pressure. Particles are elastic.
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| Kinetic Molecular Theory #3 | The particles exert no force on each other. They neither attract nor repel.
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| Kinetic Molecular Theory #4 | The kinetic energy of gas particles is directly proportional to the temperature of the gas. The particles move faster as the temperature rises.
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| Deviation from Ideal Gas | High pressure and low temperature
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| Van Der Waals's Equation | [ P + a (n/V)^2 ](V-nb) = nRT
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| Van Der Waals's Equation | P = [(nRT)/(V-nb)] - a(n/V)^2
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| Determine Final Volume (Given: V1; T1; & T2) | (V1/T1) = (V2/T2) - Charles's Law
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| Determine Final Moles (Given V1; n1; & V2) | (V1/n1) = (V2/n2) - Avogadro's Law
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| Solving with Density | Density(m/V) = [(molar mass)(P)]/RT
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| Reaction Stoichiometry | Solve for MOLES
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| Gases at Two Conditions | [(P1 X V1)/(n1 X T1)] = [(P2 X V2)/(n2 X T2)]
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| Determining Partial Pressures (double bulb diagram) | [(V X P)/Total V] + [(V X P)/Total V]
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| atm -> torr | 1 atm = 760 torr
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| Using Mole Fraction = Partial Pressure | P1/Ptotal = n1/ntotal
(n total = 1)
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| Two Reactant within a Gas Law Problem | Reactant Volume -ideal gas law-> moles of reactant - determine limiting reactant -> use limiting reactant to determine moles of product -ideal gas law-> volume of product
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| Effusion (movement) | (Rate1/Rate2) = (Molar Mass2/Molar Mass1)^1/2 ->sq root
- higher molar mass = slower rate
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| R(torr) = R(atm) = | 62.36
.0821
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| Determine Heat | Molar Heat Capacity X mol X Change in Temperature
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| Determine Energy/Heat | Specific Heat Capacity X Mass X Change in Temperature
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| Determine Specific Heat Capacity | Heat / (Mass X Change in Temperature)
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| Specific Heat Capacity | The amount of heat necessary to raise the temperature one degree of one gram of a substance
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| Determine Heat with Balanced Equation | Multiply Moles of the substance by "Delta Heat"/mole ration
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| Calorimetry | Heat loss = Heat gain
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| Calorimetry Heat Capacity | Heat Absorbed / Increase in Temp
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| Enthalpies of Formation in a Reactions | [Sum of products (moles X enthalpy formation)] - [Sum of reactants (moles X enthalpy formation)]
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| h - lambda (meters) | wavelength
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| v - nu (sec^-1 or Hz) | frequency
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| Find wavelength or frequency | lambda = constant(2.9979*10^8 m/sec) / nu
nu = constant(2.9979*10^8 m/sec) / lambda
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| Quantum Energy | Planck's constant (6.626*10^-34Js) X frequency
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| Energy of a Photon | (Planck's constant X Speed of light)/ lambda
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| Mass of a Photon | Planck's constant / (wavelength X speed of light)
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| Determine Wavelength (given mass) | Planck's constant / (mass X velocity)
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| Quantum Numbers | n; l; ml; ms
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| l numbers | 0 = s; 1 = p; 2 = d; 3 = f
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| Subshells | s = 1; p = 3; d = 5, f = 7
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| Pauli Exclusion Principle | In a given atom not two electrons can have the same set of four quantum numbers
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| Heisenberg uncertainty principle | uncertainty in particle's position X uncertainty in particle's momentum (greater than or equal to) planck's constant / 4pi
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| n | related to size and energy of the orbital
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| l | related to the shape of the orbital
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| ml | related to the position of the orbital in space relative to other orbitals
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| ms | related to the spin of the electron
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| Electron Affinity | Energy change associated with the addition of an electron
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| Ionization Energy | Energy change associated with the removal of an electron
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| Group 5 Ionization Energy | Group 5 is greater then 4 and 6
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