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