Eleanor Roosevelt High School
AP Review Questions
Answer the following multiple-choice questions to the best of your ability, using your knowledge of chemistry. Pay special attention to groups of questions that require you to refer to a specific group of answers. Comment on any work/review required for each topic (before and after checking the answers).
|Question |Topics/Skills |Comments |
|Which of the following compounds contains an element with a +1 oxidation | | |
|state? | | |
| | | |
|carbon dioxide |Oxidation numbers | |
|lead (IV) oxide | | |
|dinitrogen pentaoxide | | |
|copper (I) oxide | | |
|Questions 2-5 refer to the following chemical species: | | |
| | | |
|H2O (B) NH3 (C) BH3 (D) CH4 | | |
| | | |
|2) Has two lone pairs of electrons. |Lewis dot diagrams, VSEPR, | |
| |molecular geometry, orbital | |
| |hybridization, polarity | |
|3) Has a central atom with less than an octet of electrons. | | |
|4) Is predicted to have the largest bond angle. | | |
|5) Has a trigonal-pyramidal molecular geometry. | | |
|Questions 6-7 refer to the chemical reactions represented below: | | |
|2C6H6(l) + 15O2(g) ( 12CO2(g) + 6H2O(l) | | |
|C2H3O2-(aq) + H3O+(aq) ( HC2H3O2(aq) + H2O(l) | | |
|CaCO3(s) ( CaO(s) + CO2(g) | | |
|2 H2O2(l) ( O2(g) + 2 H2O(l) | | |
|6) The reaction between a Brønsted-Lowry acid and a Brønsted-Lowry base. | | |
| | | |
| | | |
| |Brønsted-Lowry acids and bases | |
|7) The reaction in which a single species is both oxidized and reduced. | | |
| | | |
| | | |
| |REDOX reactions | |
|Questions 8-10 refer to 1 L flasks containing each of the following, | | |
|respectively: | | |
| | | |
|Flask A: N2 (g) @ 30 °C, 1 atm | | |
|Flask B: N2 (g) @ 50 °C, 0.5 atm |KMT, IMF, macroscopic properties | |
|Flask C: O2 (g) @ 40 °C, 2 atm | | |
|Flask D: O2 (g) @ 50 °C, 1 atm | | |
| | | |
| | | |
|8) In which flask do the molecules have the greatest average speed? | | |
|9) Which flask contains the smallest number of moles of gas? | | |
| | | |
| |Moles and gases | |
|10) Which flask contains the sample with the greatest density? | | |
| |Mathematical principles/macroscopic| |
| |properties | |
|11) Which of the following elements has the largest first ionization energy? | | |
| |Periodic properties: ionization | |
|(A) Li (B) Be (C) B (D) N |energy | |
|12) A 0.20 mol sample of MgCl2 (s) and a 0.10 mol sample of KCl(s) are | | |
|dissolved in water and diluted to 500 mL. What is the concentration
of Cl- in |Comparisons of numbers of | |
|the solution? |particles, moles, masses, and | |
| |volumes | |
|(A) 0.15 M (B) 0.30 M (C) 0.60 M (D) 1.0 M | | |
| | | |
| | | |
|13) Atoms of Mg combine with atoms of F to form a compound. Atoms of which of | | |
|the following elements combine with atoms of F in the same ratio? | | |
| |Periodic properties: reactivity | |
|(A) Li (B) Ba (C) Al (D) Cl | | |
|14) How many protons, neutrons, and electrons are in an iron-56 atom? | | |
| |Subatomic particles in an atom | |
|(A) 26, 30, 26 (C) 30, 26, 30 |(isotope or ion) | |
|(B) 26, 56, 26 (D) 56, 26, 26 | | |
|15) In the reaction represented below, what is the total number of moles of | | |
|reactants consumed when 1.00 mole of CO2 (g) is produced? | | |
| | | |
|C3H8(g) + 5 O2(g) ( 3 CO2(g) + 4 H2O(l) |Stoichiometric calculations | |
|(A) 0.33 (B) 1.33 (C) 1.50 (D) 2.00 | | |
| | | |
|16) Which of the following is the electron configuration of an excited atom | | |
|that is likely to emit a quantum of energy? | | |
| | | |
|1s2 2s22p6 3s23p1 | | |
|1s2 2s22p6 3s23p5 | | |
|1s2 2s22p6 3s2 |Distribution of electrons, | |
|1s2 2s22p6 3s13p1 |Coulomb’s Law, electron energies | |
|17) Which of the following molecules contains polar covalent bonds but is a | | |
|nonpolar molecule? |Lewis dot diagrams, VSEPR, | |
| |molecular geometry, orbital | |
|CH3Cl (B) NH3 (C) CCl4 (D) N2 |hybridization, polarity | |
|18) In the reaction represented below, what
mass of HF is produced by the | | |
|reaction of 3.0 × 1023 molecules of H2 with excess F2? (Assume the reaction | | |
|goes to completion.) | | |
| | | |
|H2 + F2 ( 2HF | | |
| |Stoichiometric calculations | |
| | | |
|(A) 1.0 g (B) 4.0 g (C) 10. g (D) 20. g | | |
| | | |
| | | |
| | | |
|19) For which of the following reaction mixtures at equilibrium would reducing| | |
|the volume of the container at constant temperature cause the equilibrium to | | |
|shift toward the products? | | |
| | | |
|SrCO3(s) ( SrO(s) + CO2(g) | | |
|C(s) + CO2(g) ( 2 CO(g) | | |
|CO(g) + H2O(g) ( CO2(g) + H2(g) |LeChatelier’s Principle | |
|2 NO2(g) ( N2O4(g) | | |
|20) A 2 L sample of N2 (g) and a 1 L sample of Ar(g), each originally at 1 atm| | |
|and 0°C, are combined in
a 1 L tank. If the temperature is held constant, | | |
|what is the total pressure of the gases in the tank? |Mathematical relationships/gases | |
| | | |
|(A) 1 atm (B) 2 atm (C) 3 atm (D) 4 atm | | |
|21) Which of the following processes involves the greatest increase in | | |
|entropy? | | |
| | | |
|SO3(g) + H2(g) ( SO2(g) + H2O(g) | | |
|Ag+(aq) + Cl -(aq) ( AgCl(s)
| | |
|C2H2(g) + 2 H2(g) ( C2H6(g) |Entropy | |
|MgSO (s) ( MgO(s) + SO (g) | | |
|22) N2O5(g) ((2 NO2(g) + 1/2 O2(g) | | |
|The equilibrium constant for the gas phase reaction above is 95 at 25 °C. What| | |
|is the value of the equilibrium constant for the following reaction
at 25 °C?| | |
|O2(g) + 4 NO2(g) ((2 N2O5(g) | | |
|(95)2 (B) 95 (C) 1/95 (D) 1/(95)2 | | |
| | | |
| |Manipulation of equilibrium | |
| |constant | |
|23) C2H4(g) + H2(g) + Pt (catalyst) (C2H6(g) | | |
|C2H4(g) is reduced by H2(g) in the presence of a solid platinum catalyst, as | | |
|represented by the equation above. Factors that could affect the rate of the | | |
|reaction include which of the following? | | |
|Changes in the partial pressure of H2(g) | | |
|Changes in the particle size of the platinum catalyst | | |
|Changes in the temperature of the reaction system |Interpreting the results of an | |
|I and II (B) I and III (C) II and III (D) all |experiment based on rate changes | |
|24) For an experiment, a student needs 100.0 mL of 0.4220 M NaCl. If the | | |
|student starts with NaCl(s) and distilled water, which of the following pieces| | |
|of laboratory glassware should the student use to prepare the solution with | | |
|the greatest accuracy? | | |
| | | |
|25 mL volumetric pipet |Experimental design | |
|100 mL Erlenmeyer flask | | |
|100 mL graduated cylinder | | |
|100 mL volumetric flask | | |
|25) 2NH3 (g) → 3H2 (g) + N2 (g) Δ H° = 92 kJ/mol | | |
|According to the information above, what is the standard enthalpy of | | |
|formation, Δ H°, for NH3 (g) at 298 K (in kJ/mol)? | | |
|(A) -92 (B) -46 (C) 46 (D) 92 |Reaction enthalpy | |
|26) The percentage of silver in a solid sample is determined gravimetrically | | |
|by converting the silver to Ag+ (aq) and precipitating it as silver chloride. | | |
|Failure to do which of the following could cause errors in the analysis? | | |
| | | |
|Account for the mass of the weighing paper when determining the mass of the | | |
|sample | | |
|Measure the temperature during the precipitation reaction | | |
|Wash the precipitate | | |
|Heat the AgCl precipitate to constant mass |Experimental design | |
|(A) I & II (B) I & IV (C) II & III (D) I, III, & IV | | |
|27) The reaction represented below is observed to proceed spontaneously to the| | |
|right in aqueous solution. What is the strongest base in the system? | | |
| |Equilibrium constant/acid-base | |
|HSO4-(aq) + CO32-(aq) (SO42-(aq) + HCO3-(aq) |theory | |
|(A) sulfate (B) carbonate (C) water (D) hydrogen carbonate | | |
|28) When the equation below is balanced and the coefficients are reduced to | | |
|lowest
whole-number terms, what is the coefficient of H2O(l)? | | |
|LiHCO3(aq) + H2SO4(aq) ( Li2SO4(aq) + H2O(l) + CO2(g) | | |
|(A) 1 (B) 2 (C) 3 (D) 4 | | |
| |Balancing equations | |
|29) Which of the following lists the substances F2, HCl, and HF in order of | | |
|increasing boiling point? | | |
| |Phases of matter/IMF | |
|(A) HF < HCl < F2 (C) HCl < F2 < HF | | |
|(B) HF < F2 < HCl (D) F2 < HCl < HF | | |
|30) Gases generated in a chemical reaction are sometimes collected by the | | |
|displacement of water, as shown to the right. Which of the following gases can| | |
|be quantitatively collected by this method? | | |
| | | |
|(A) H2 (B) CO2 (C) HCl (D) NH3 | | |
| | | |
| |Solubility of gases in water | |
|31) When a 3.22 g sample of an unknown hydrate
of sodium sulfate, Na2SO4 x H2O| | |
|(s), is heated, H2O (molar mass 18 g) is driven off. The mass of the anhydrous| | |
|Na2SO4(s) (molar mass 142 g) that remains is 1.42 g. The value of x in the |Applying mathematical routines to | |
|hydrate is |mass data | |
| | | |
|(A) 0.013 (B) 1.8 (C) 6.0 (D) 10. | | |
| | | |
|32) A 0.10 M solution of a weak monoprotic acid has a pH equal to 4.0. The | | |
|ionization constant, Ka, of the acid is |Calculating pH of a weak acid | |
| | | |
|(A) 1x 10-3 (B) 1 x 10-4 (C) 1x 10-7 (D) 1 x 10-8 | | |
|33) In an insulated cup of negligible heat capacity, 50. g of water at 40.°C | | |
|is mixed with 30. g of
water at 20.°C. The final temperature of the mixture |Conservation of energy/magnitudes | |
|is closest to |of energy changes | |
|(A) 27 °C (B) 30 °C (C) 33 °C (D) 38 °C | | |
|34) Which of the following is an isomer of CH3OCH3? | | |
| | | |
|(A) CH3CH3 (C) CH3CH2OH |Isomers | |
|(B) CH3COOH (D) CH3CH2CH3 | | |
| | | |
| | | |
| | | |
|35) Potassium hydrogen phthalate, KHP, is used as a primary standard for | | |
|determining the concentration of a solution of NaOH by titration. If the KHP | | |
|has not been dried before weighing, the calculated molarity of the NaOH would | | |
|be | | |
| | | |
|higher than the actual value, since water is included in the apparent mass of | | |
|KHP | | |
|higher than the actual value, since the presence of water requires a larger |Experimental design: titrations | |
|volume of titrant | | |
|lower than the actual value, since NaOH absorbs water | | |
|unaffected, since KHP is a strong acid | | |
|36) Which of the following substances has the greatest solubility in C5H12(l) | | |
|at 1 atm? | | |
| |Solubility/IMF | |
|(A) SiO2 (s) (B)NaCl (s) (C) H2O (l) (D) CCl4 (l) | | |
| | | |
|37) The data in the table below were obtained for the reaction X + Y ( Z. | | |
|Which of the following is the rate law for the reaction? | | |
| | | |
|Experiment [X]0 [Y]0 Rate of Formation Z | | |
|1 0.10 M 0.30 M 4.0 x 10-4 | | |
|2 0.20 M 0.60 M 1.6 x 10-3 |Rate laws | |
|3 0.20 M 0.30 M 4.0 x 10-4 | | |
| | | |
|rate = k[X]2 (C) rate = k[X][Y] | | |
|rate = k[Y]2 (D) rate = k[X]2[Y] | | |
| | | |
| | | |
|38) For the reaction represented above at 25 °C, what
are the signs of ΔH°, | | |
|ΔS°, and ΔG°, respectively? | | |
|(A) +, +, + (B) +, +, - (C) -, -, - (D) -, -, + |Thermodynamics, spontaneity | |
| | | |
|39) What is the empirical formula of an oxide of chromium that is 48 percent | | |
|oxygen by mass? | | |
| |Mathematical data: empirical | |
|(A) CrO (B) CrO2 (C) CrO3 (D) Cr2O3 |formulas | |
| | | |
|40) High solubility of an ionic solid in water is favored by which of the | | |
|following conditions? | | |
| | | |
|The existence of strong ionic attractions in the crystal lattice. | | |
|The formation of strong ion-dipole attractions. | | |
|An increase in entropy upon dissolving |Coulomb’s Law/IMF | |
|(A) I (B) I & II (C) I & III (D) II & III | | |
|41) Which of the following statements is true for the equilibrium vapor | | |
|pressure of a liquid in a closed system? | | |
| | | |
|It remains constant when the temperature increases. | | |
|It decreases to half its original value if the volume of the gas phase is | | |
|doubled. |LeChatelier’s Principle/vapor | |
|It increases to twice its original value if the volume of the liquid phase is |pressure | |
|doubled. | | |
|It is independent of the volume of the vapor phase. | | |
|42) An unknown acid is dissolved in 25 mL of water and titrated with 0.100 M | | |
|NaOH. The equivalence point of the titration is approximately 8.0. Which of |Titration weak acid/strong base; pH| |
|the following could be the unknown acid? |determination of equivalence point | |
| | | |
| | | |
|Fluoroacetic acid, pKa = 2.6 | | |
|Glycolic acid, pKa = 3.8 | | |
|Propanoic acid, pKa = 4.9 | | |
|Hypochlorous acid, , pKa = 7.5 | | |
| | | |
|43) Which of the following lists Mg, P, and Cl in order of increasing atomic | | |
|radius? |Periodic properties: atomic | |
| |structure | |
|(A) Cl < P < Mg (C) Mg < P < Cl | | |
|(B) Cl < Mg < P (D) Mg < Cl < P | | |
| | | |
|44) When 4.00 mol each of X(g) and Y(g) are placed in a 1.00 L vessel and | | |
|allowed to react at constant temperature according to the equation below, 6.00| | |
|mol of Z(g) is produced. What is the value of the equilibrium constant, Kc? | | |
| |Properties of equilibrium given | |
|X (g) + Y (g) (( 2Z (g) |data | |
| | | |
|(A) 3 (B) 8 (C) 16 (D) 36 | | |
| | | |
|45) If the oxygen isotope 20O has a half-life of 15 seconds, what fraction of | | |
|a sample of pure 20O remains after 1.0 minute? | | |
|(A) ½ (B) ¼ (C) 1/8 (D) 1/16 |Half-life, rate constant | |
| | | |
|46) Pure substance X decomposes according to the equation following equation X| | |
|( products. Which of the following graphs indicates that the rate of | | |
|decomposition is second order in X? | | |
| | | |
|(A) [pic] (C) [pic] | | |
| |Graphical analysis of concentration| |
|(B) [pic] (D) [pic] |vs. time | |
|47) Permanganate and oxalate ions react in an acidified solution according to | | |
|the balanced equation below. How many moles of CO2 (g) are produced when 20. | | |
|mL of acidified 0.20 M KMnO4 solution is added to 50. mL of 0.10 M Na2C2O4 | | |
|solution? | | |
| | | |
|2 MnO4- (aq) + 5 C2O42- (aq) + 16 H+ (aq) → 2 Mn2+ (aq) + 10 CO2 (g) + |Stoichiometry: predicting results | |
|8 H2O(l) |of reaction | |
| | | |
|(A) 0.0040 mol (C) 0.010 mol | | |
|(B) 0.0090 mol (D) 0.020 mol | | |
| | | |
| | | |
|48) A student is trying to determine the heat
of reaction for the acid-base | | |
|neutralization reaction represented below. The student uses 0.50 M NaOH and | | |
|0.50 M HCl solutions. Which of the following situations, by itself, would most| | |
|likely result in the LEAST error in the calculated value of the heat of | | |
|reaction? | | |
| | | |
|NaOH (aq) + HCl (aq) ( H2O (l) + NaCl (aq) | | |
| |Experimental design: calorimetry | |
|The thermometer was incorrectly calibrated and read 0.5 Celsius degree too | | |
|high during the procedure. | | |
|The volume of the acid solution added to the calorimeter was actually 1.0 mL | | |
|less than what was recorded. | | |
|The calorimeter was poorly insulated, and some heat escaped to the atmosphere | | |
|during the procedure. | | |
|The actual molarity of the base solution was 0.53 M but was recorded as 0.50 | | |
|M. | | |
|49) A molecular solid coexists with its liquid phase at its melting point. The| | |
|solid-liquid mixture is heated, but the temperature does not change while the | | |
|solid is melting. The best explanation for this phenomenon is that the heat | | |
|absorbed by the mixture | | |
| | | |
|is lost to the surroundings very quickly | | |
|is used in overcoming the intermolecular
attractions in the solid
|Heat capacity/energy changes | |
|is used in breaking the bonds within the
molecules of the solid
| | |
|causes the nonbonding electrons in the
molecules to move to lower energy | | |
|levels | | |
|50) The role of a catalyst in a chemical reaction is to | | |
| | | |
|decrease the amount of reactants that must be used | | |
|lower the activation energy for the reaction | | |
|supply the activation energy required for the
reaction to proceed
|Catalysts and reaction rates | |
|increase the amounts of products formed at
equilibrium
| | |
|51) If 50. mL of 1.0 M NaOH is diluted with distilled water to a volume of 2.0| | |
|L, the concentration of the resulting solution is |Quantitative connection of | |
| |substances | |
|(A) 0.025 M (B) 0.050 M (C) 0.50 M (D) 1.0 M | | |
| | | |
|52) Which of the following is NOT an accepted name for the formula given? | | |
| | | |
|CH3OH… methanol |Nomenclature | |
|CuO… copper (I) oxide | | |
|FeCl3… iron (III) chloride | | |
|SrCO3… strontium carbonate | | |
| | | |
|53) Which of the following molecules contains exactly three sigma bonds and | | |
|two pi bonds? | | |
| |Lewis dot diagrams/bond theory | |
|C2H2 (B) CO2 (C) SO3 (D) N2 | | |
| | | |
|54) Resonance is most commonly used to describe the bonding in molecules of | | |
|which of the following? |Lewis dot diagrams/bond theory55) | |
| | | |
|(A) CO2 (B) O3 (C) H2O (D) SF6 | | |
|55) A student prepares a solution by dissolving 60.00 g of glucose (molar mass| | |
|180.2 g/mol) in enough distilled water to make 250.0 mL of solution. The | | |
|molarity of the solution should be reported as |Quantitative comparison of | |
| |substances | |
|(A) 12.01 M (B) 12.0 M (C) 1.332 M (D) 1.33 M | | |
|56) Which of the following substances is a strong electrolyte when dissolved | | |
|in water? |Electrolytes; solute/solvent | |
| |interactions | |
|(A) sucrose (C) sodium nitrate | | |
|(B) ethanol (D) acetic acid | | |
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