Ap Chemistry Review – Flashcards
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| endothermic |
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| transfers thermal energy from surrounding (cold) |
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| exothermic |
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| transfers thermal energy to surroundings (warm) |
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| Graham's Law of Effusion |
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| rate of effusion UF6/ rate of effusion H2 square root of mm of UF6/H2 always put the lower molar mass at the bottom |
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| Dalton's Law of Partial Pressure |
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| n=PV/RT 25C He (1)(46)/(.0821)(298)= 1.9 mols O2 (1)(12)/(.0821)(298)= .49 mols P=nRT/V He (1.9)(.0821)(298)/(5)= 9.3 atms O2 (.49)(.0821)(298)/(5)= 2.4 atms Total= 9.3 + 2.4 = 11.7 atms |
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| Avogadro |
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| the volume is proportional to the number of moles. As the moles increase, the volume increase. V1 / N1 = V2 / N2 |
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| Gay-Lussac |
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| temperature is directly related to pressure. As temperature increases, pressure increases P1 / T1 = P2 / T2 |
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| Charles |
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| volume is directly proportional to the temperature. When temperature decrease volume decreases V1 / T1 = V2 /T2 |
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| Boyle |
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| volume is inversely related to pressure. As pressure increases, volume increases. P1 * V1 = P2 * V2 |
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| acids |
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| proton donor strong acids - HCl - HNO3 - H2SO4 - HClO4 weak acids - HC2H3O2 - HF - H3PO4 |
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| bases |
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| proton acceptor strong bases - NaOH - Ba(OH)2 weak bases - NH3 |
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| molarity |
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| moles / liters = M |
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| percentage yield |
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| part / whole *100 OR actual yield / theoretical yield *100 |
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| limiting reagent |
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| 1) balance the equation 2) convert grams to mass grams / molar mass 3) to determine limiting reagent, use mole ratio 4) use stoichiometry |
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| determining formulas |
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| given 40.92% C - 4.58% H - 54.5% O 1) percent / molar mass 2) divide all numbers by lowest number 3) * by a number to get whole numbers answer = C3H4O3 |
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| naming acids |
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| without oxygen - prefix - hydro... suffix - ...ic HCl - hydrochloric acid HCN - hydrocyanic acid with oxygen - no prefix anion is ...ate, suffix - ... ic anion is ...ite, suffix - ... ous HNO3 - nitric acid H2SO3 - sulfurous acid |
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| radiant energy |
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| aka solar energy, comes from the sun and is Earth's primary source of energy. It consists if the electromagnetic spectrum from radio to gamma waves. |
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| thermal energy |
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| is the energy associated with the random motions of atoms and molecules. In general, thermal energy can be calculated from temperature. |
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| chemical energy |
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| is stored within the structural units of chemical substances, ie bonds. |
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| kinetic energy |
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| is associated with moving objects, ie thermal. |
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| potential energy |
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| is associated with an objects position, ie chemical. |
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| standard heat of formation |
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| products - reactants |
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| DeBroglie |
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| a wave can behave like a particle. |
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| Heisenberg |
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| it is impossible to know simultaneously both the momentum and position of a particle with uncertainty |
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| four quantum numbers |
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| 1) n, average distance if the electron larger n, further from the nucleus 2) s=0 p=1 d=2 f=3 shape of the orbital 3) ml, 2p has 3, 2p orbitals value of ml are -1, 0, 1 4) ms, spin of quantum number -1/2, 1/2 |
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| Aufbau |
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| electrons enter orbitals of lowest energy first. |
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| Pauli |
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| each orbital may contain only 2 electrons and they each must have an opposite spin. |
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| Hund |
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| electrons occupy orbitals of equal energy. |
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| ionization energy |
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| minimum energy required to remove an electron from a gaseous atom. radius increases when we move down a group because the nuclear charge attracts electrons. |
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| ionic bonds |
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| a non metal takes valence electrons from a metal. This creates two atoms with opposite charges and opposites attract. |
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| covalent bonds |
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| a pair of valence electrons are shared between 2 non metal atoms |
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| metallic bonds |
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| electrons are shared by being passed on from metal to metal atom. |
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| intermolecular force |
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| stickiness to keep the molecules of a liquid cling together. |
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| mass percent |
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| mass of solute / mass of solution * 100 |
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| if a gas occupies 14.2 liters of space at STP, how many moles of gas are present? |
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| 14.2 liters / 22.414 liters = .634 moles |
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| calculate the volume of N2 generated at 80C and 823 mm Hg by the decomposition of 60 g of NaN3 |
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| 2NaN3 → 2Na + 3N2 60 g NaN3/65.02 g NaN3*3 / 2 =1.38 mols N2 PV=nRT (823/760) V = 1.38* .08206 * 353 V= 36.9 liters |
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| what is the molarity of a solution prepared by dissolving 11.5 g of NaOH in enough water to make 1.5 liters of solution? |
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| (1/1.5) * (11.5/1) * (1/40.0) = .192 M |
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| how many grams of CuSO4 are contained in 500. ml of .750 M CuSO4 solution? |
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| (.500/1) * (.750/1) * (159.61/1) = 59.9 g |
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| when 1.liter of 1.M Ba(NO3)2 solution at 25C is mixed with 1.liter of 1.M NaSO4 solution at 25C forms the temp of 28.1C Calculate the enthalpy Δ per mol of BaSO4 formed. |
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| Q = m s Δ T mass of solution 2.00 * 1000 * 1.0 = 2.0*10^3 ΔT = 28.1 - 25 = 3.1C ΔH = 4.18* (2.0*10^3) * 3.1C = 2.6*10^4 exothermic, ΔH = 2.6*10^4 J -26KJ |
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| find the pH of .0180M (OH) 5.6 *10^4 |
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| (H) = 1.0*10^-14 / 5.6*10^.4 = 1.8*10^-11 pH = -log (H) = 10.7 or (OH) 5.6*10^-4 pOH = 3.252 14.00 - 3.252 = 10.7 |
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| determine the percent ionization of NH3 in .0180 M NH3 (OH) 5.6*10^-4 in .0180 M NH3 25C |
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| 5.6*10^-4 / .0180 * 100% = 3.11% |
