Chemistry 101 Practice Final Exam Key PDF

Name: Section: Use only the equation sheets given to you from exam 1. Try to answer the questions without looking at your book, notes, or the internet. Treating this review as a real exam will give you a more accurate indicator of the topics you shoul...

Name: Section: Use only the equation sheets given to you from exam 1. Try to answer the questions without looking at your book, notes, or the internet. Treating this review as a real exam will give you a more accurate indicator of the topics you should focus more on. The following 30 questions are based on material from chapters 10 and 11. 1. Which of the following is not a condition listed in the kinetic theory of reactions? A collisions must have enough energy B molecules must collide to react C collisions must have correct orientation D molecules must be stationary 2. Which of the following below correctly defines the function of a catalyst? A It increases the activation energy B It slows down the rate of a reaction C It is used up during a reaction D None of the above E All of the above 3. A reversible reaction is at equilibrium when A only the rate of the forward reaction changes B the reaction rate of the forward and reverse reaction are not constant C the forward reaction rate equals the reverse D only the rate of the reverse reaction changes reaction rate 4. What is the equilibrium constant for the following reaction if the mixture contains 0.31 M CO2, 0.029 M H2, 0.25 CO, and 0.27 M H2O? CO2 (g) + H2 (g) ↔ CO (g) + H2O (g) A 0.13 B 0.86 C 6.4 D 7.5 5. For the following equation, what is the proper from of the equilibrium expression? 2BrNO (g) ↔ Br2 (g) + 2 NO (g) A B C D -1- Chemistry 101 Final Exam Practice  6. For the reaction N2O4 (g) ↔ 2 NO2 (g) the equilibrium constant is 4.3 x 10-3. If the equilibrium mixture contains [NO2] = 0.053 M, what is the molar concentration of N2O4? A 12 M B 1.5 M C 0.65 M D 0.081 M 7. Which of the following equilibrium constants would indicate an equilibrium mixture that contains mostly reactants? A 7.2 x 102 B 5.0 x 109 C 6.0 x 1023 D 1.0 x 10-95 8. An equilibrium constant greater than 1 indicates that a reaction mixture at equilibrium most likely contains A Mostly reactants B Mostly products C Equal amount of reactants and products D Double the amount of reactants than products 9. The Kc for the following reaction is 1.7 x 102 at 225 °C. If the equilibrium mixture contains 0.18 M H2, and 0.020 M N2, what is the molar concentration of NH3? 3H2 (g) + N2 (g) ↔ 2NH3 (g) A 0.14 M B 0.63 M C 0.25 M D 0.31 M 10. For the reaction CO (g) + H2O (g) ↔ CO2 (g) + H2 (g) + Heat, if the temperature is decreased, where does the equilibrium shift? A Shifts right towards the products B Shifts left towards the reactants C Does not change 11. Using the same equation from question 10, if H2 (g) is added, where does the equilibrium shift? A Shifts right towards the products B Shifts left towards the reactants C No change 12. Consider the following reactions, which reaction's equilibrium would not change if the volume of the container was doubled? A 2NH3 (g) ↔ 3H2 (g) + N2 (g) B N2 (g) + O2 (g) ↔ 2NO (g) C N2 (g) + 2O2 (g) ↔ 2NO2 (g) D 4NH3 (g) + 3O2 (g) ↔ 2N2 (g) + 6H2O (g) 13. For the following reaction C2H4 (g) + Cl2 (g) ↔ C2H4Cl2 (g) + Heat, if a catalyst is added, where the does the equilibrium shift? A Shifts right towards the products B Shifts left towards the reactants C No change -2- Chemistry 101 Final Exam Practice 14. Out of the choices listed, what is true about KOH? A It is a proton donor B It would most likely have a sour taste C It would increase the pH of a solution D It is a good source of hydronium ions 15. Name the following acid, H3PO4 A Phosphatic acid B Trihydrogen phosphoric acid C Phosphorous acid D Phosphoric acid 16. What is the correct formula for the base, aluminum hydroxide? A AlOH B Al2OH C Al(OH)3 D Al3OH 17. For the following equation identify the Bronsted-Lowry acid and the Bronsted-Lowry base NH3 (aq) + H2O (l) ↔ NH4+ (aq) + OH- (aq) A NH3 is the acid (proton donor), H2O is the base B H2O is the acid (proton donor), NH3 is the base (proton acceptor) (proton acceptor) C NH3 is the acid (proton acceptor), H2O is the D H2O is the acid (proton acceptor), NH3 is the base (proton donor) base (proton donor) 18. Identify the conjugate acid/base pairs in the equation (the answer should be in order of acid then base for each pair): H2SO4 (aq) + H2PO4- (aq) ↔ HSO4- (aq) + H3PO4 (aq) A HSO4-/H2SO4 and H3PO4/H2PO4- B H2SO4/HSO4- and H2PO4-/H3PO4 C HSO4-/H2SO4 and H2PO4-/H3PO4 D H2SO4/HSO4- and H3PO4/H2PO4- 19. Identify if the equilibrium mixture from the previous question contains mostly reactants, products, or an equal amount of both. Assume H2SO4 has a pKa 1. A Contains mostly products B Contains mostly reactants C Contains and equal amount of reactants and products 20. Identify the strongest acid out of the choices listed below. A Acetic acid (Ka= 1.76 x 10-5) B Nitrous acid (Ka= 7.2 x 10-4) C Hydroiodic acid (Ka= 3.2 x 109) D Sulfuric acid (Ka= 1.0 x 103) -3- Chemistry 101 Final Exam Practice 21. Identify what is not true about weak acids A They have a small Ka value B They have a large pKa C They dissociate only slightly in aqueous D They have a weak conjugate base solutions 22. What is the pH of a solution that has a [OH-] = 1.5 x 10-6 M? A 5.8 B 8.2 C 6.0 D 9.1 23. What is the concentration of [H3O+] with a pH of 6.5? A 6.5 x 10-10 M B 4.1 x 10-10 M C 3.2 x 10-7 M D 1.0 x 10-7 M 24. What is the pH of a solution with a pOH of 4.3? A 4.3 B 9.7 C 7.9 D 3.4 25. The answer to the previous question would have a solution that is A Basic B Neutral C Acidic 26. In the reaction between KHCO3 (s) and HBr (aq), what gas is produced? A H2 (g) B CO2 (g) C O2 (g) D H2O (g) 27. A solution of 0.621 M H3PO4 is used to titrate 10.0 mL of a 0.431 M KOH solution. What volume, in milliliters, of H3PO4 solution is required? H3PO4 (aq) + 3KOH ↔ 3H2O (l) + K3PO4 (aq) A 0.0144 mL B 0.0480 mL C 2.31 mL D 10.0 mL 28. What is the molarity of the acetic acid solution if 34.7 mL of a 0.235 M KOH is required to titrate 26.0 mL of a solution of HC2H3O2 (acetic acid)? HC2H3O2 (aq) + KOH (aq) ↔ H2O (l) + KC2H3O2 (aq) A 0.625 M B 0.521 M C 0.314 M D 0.127 M -4- Chemistry 101 Final Exam Practice 29. What is the pH of a buffer solution containing 0.17 M HC2H3O2 (acetic acid) and 0.19 M C2H3O2-? Acetic acid Ka = 1.8 x 10-5. A 4.79 B 4.54 C 4.31 D 4.85 30. What is the purpose of a buffer? A To maintain pH B To increase pH C To decrease pH D To neutralize pH The following 20 questions are the cumulative portion of the exam. 31. What is the density of a medication if 16.5 mL has a mass of 42.9 g? A 26.4 g-mL B 2.60 g/mL C 0.385 mL/g D 708 g mL 32. A cube of silver with a density of 10.5 g/cm3, has a volume of 19.0 cm3. Calculate the energy needed for the temperature of the cube to go from 16 °C to 24 °C. The specific heat for silver is 0.0562 cal/g·°C. A 200 cal B 125 cal C 90 cal D 75 cal 33. Calculate the total kilojoules in two tablespoons of crunchy peanut butter that contains 4g carbohydrates, 13g fat, and 7g proteins. A 900 kJ B 680 kJ C 240 kJ D 160 kJ 34. Calculate the heat change in kJ for melting 170g of ice at 0°C. A 14 kJ B 29 kJ C 57 kJ D 80 kJ 35. Energy stored in an object due to its position (like a holding a ball 5 feet above the ground) is an example of A Potential energy B Kinetic energy C Positional energy D Chemical energy -5- Chemistry 101 Final Exam Practice 36. What type of nuclear reaction is represented in the balanced equation pictured above? A Bombardment B Beta decay C Fission reaction D Alpha decay 37. Which element has the electron configuration 1s22s22p3? A Carbon B Sulfur C Magnesium D Nitrogen 38. Which of the following elements has the smallest atomic radius? A Kr B Ca C K D Br 39. Using VSEPR theory NI3 has what shape? A trigonal planar B bent C trigonal pyramidal D linear 40. Which is the correct Lewis dot structure for BF4-? A B C D -6- Chemistry 101 Final Exam Practice 41. For the following reaction, how much product would you produce if you had 32.0 g of each reactant? 4Cr (s) + 3O2 (g) → 2Cr2O3 (s) A 101.3 g B 93.5 g C 64.0 g D 46.8 g 42. Using your answer from the previous question, if you actually produced 16.3 g of product, what is the percent yield? A 34.8% B 25.5% C 17.4% D 16.1% 43. How many kilojoules are released when 68.7g of oxygen reacts? 2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l) ΔH = -726 kJ A 520 kJ B 1500 kJ C 730 kJ D 16000 kJ 44. The air in a 4.00 L tank has a pressure of 2.0 atm. What is the final pressure, in mmHg, if the volume in the tank is decreased to 1.18 L? A 6.78 mmHg B 5150 mmHg C 9.47 mmHg D 2730 mmHg 45. Calculate the number of equivalents (Eq) for 3 moles of Fe3+. A 1 Eq B 3 Eq C 6 Eq D 9 Eq 46. Which of the following ionic compounds are soluble in water? A Na3PO4 B Ag2S C BaSO4 D Zn3(PO4)2 47. What is the final concentration if 3.5 L of a 4.0 M HNO3 solution is added to water so that the final volume is 8.0 L? A 0.75 M B 1.8 M C 0.57 M D 2.1 M 48. Two colloid solutions, a 0.75% (m/v) albumin solution and a 3.0% (m/v) albumin solution, are separated by a semipermeable membrane. Which compartment has the highest osmotic pressure? A 0.75% (m/v) albumin solution B 3.0% (m/v) albumin solution C Neither -7- Chemistry 101 Final Exam Practice 49. 2.01 moles of glucose (C6H12O6) is added to 1.00 kg of water. Calculate the boiling point of the solution. A 100.01 °C B 101.03 °C C 107.06 °C D 102.02 °C 50. What is the solid formed when you mix LiNO3 (aq) with Na2CO3 (aq)? A Li2CO3 B NaNO3 C No reaction -8- Chemistry 101 Final Exam Practice