<p> Chemistry CPA Final Exam Study Guide Final Exam Date: Wednesday, June 18, 2014 Exam Time: 10:15 – 12:00 pm</p><p>Topic List</p><p>Chemical Reactions  Parts of a reaction  Identify the types of reactions  Balance  Write the formula equation if you are given a word equation</p><p>Mole  Molar Mass  Convert moles-grams and grams-moles  Percent Composition  Stoichiometry  Limiting Reactant  Percent Yield</p><p>Solutions  Solubility Curves  Molarity</p><p>Gas Laws and KMT  Kinetic Molecular Theory  Heating/Cooling Curves  Boyle  Charles’  Gay-Lussac  Ideal</p><p>Acid/Base  Properties  Calculate pH and pOH and find [H+] and [OH-] </p><p>Exam Structure</p><p> o Part 1 = 80 points: Multiple choice questions o Part 2 = 20 points: Open-Ended/Free Response</p><p>Chemistry CPA Final Exam Study Guide - 2014 1 Callahan, Pengitore & Ricafort You will be given the following formula sheet and a periodic table. Mole Conversion</p><p>Given unit x ______</p><p>Given unit</p><p>Percent Composition = Mass of element x 100 Molar mass</p><p>Percent yield = actual x 100 theoretical </p><p>Gas laws</p><p>Temperature in Kelvin = °C + 273</p><p>P1V1=P2V2 T1V2 = T2V1 T1P2 = T2P1</p><p>PV = nRT, where R = 0.0821</p><p>Molarity</p><p>Acids & Bases pH + pOH = 14 pH = - log [H+] pOH = - log [OH-]</p><p>2 Unit 5: Chemical Reactions</p><p>1. What does the law of conservation of mass state?</p><p>2. Why is it necessary to balance a chemical equation?</p><p>3. What is the difference between a word equation and a chemical equation? Give an example of each. </p><p>Complete the chart</p><p>Symbol Explanation</p><p>Used to separate two reactants or two products</p><p>Yields, separates reactants and products</p><p>States of matter; Fe (s) </p><p>Aqueous solution – dissolved in water</p><p>Chemistry CPA Final Exam Study Guide - 2014 3 Callahan, Pengitore & Ricafort 4. Identify the type of reaction and balance the reaction.</p><p>A) ____ NaBr + ____ Ca(OH)2  ___ CaBr2 + ____ NaOH</p><p>Type of reaction: ______</p><p>B) ____ NH3+ ____ H2SO4  ____ (NH4)2SO4 </p><p>Type of reaction: ______</p><p>C) ____ C5H9O + ____ O2  ____ CO2 + ____ H2O</p><p>Type of reaction: ______</p><p>D) ____ Pb + ____ H3PO4  ____ H2 + ____ Pb3(PO4)2</p><p>Type of reaction: ______</p><p>E) ____ Li3N + ____ NH4NO3  ___ LiNO3 + ___ (NH4)3N</p><p>Type of reaction: ______</p><p>F) ____ HBr  ____H2 + ____Br2</p><p>Type of reaction: ______</p><p>4 5. Balance the reaction: Ag + HNO3  AgNO3 + H2O + NO2</p><p>A. 1:1:1:1:1</p><p>B. 2:2:2:2:1</p><p>C. 2:1:2:2:2 </p><p>D. 1:2:1:1:1</p><p>E. none</p><p>6. Given the following word equations, right a formula equation. Then identify the type of reaction:</p><p>A. Sodium metal and chlorine gas react to form sodium chloride crystals</p><p>B. propane gas and oxygen gas react to form carbon dioxide, water vapor, and energy. </p><p>C. zinc metal reacts with hydrochloric acid to form zinc chloride solution and hydrogen gas. </p><p>Lab Questions: Know/be able to do:</p><p> Know the signs of a chemical reaction  Know the five classifications of a chemical reaction  Know the activity of metals</p><p>Chemistry CPA Final Exam Study Guide - 2014 5 Callahan, Pengitore & Ricafort Unit 6: Moles </p><p>Match each item with the correct statement below. a. particle b. mole c. Avogadro's number 6.02 x 1023 d. percent composition</p><p>7. ______the number of particles of a substance present in 1 mole of that substance</p><p>8. ______A term to describe an atom, ion, or a molecule</p><p>9. ______the SI unit used to measure amount of substance</p><p>10. ______the percent by mass of each element in a compound</p><p>Molar Mass (use your periodic table)</p><p>11. What is the molar mass of AuCl3?</p><p>12. What is the molar mass of (NH4)2CO3</p><p>13. What is the molar mass of barium?</p><p>6 Moles and Mass (use the molar mass to convert to moles or grams)</p><p>14. What is the mass in grams of 5.90 moles of C8H18</p><p>15. What is the mass in grams of 9.32 moles of He?</p><p>16. What is the number of moles in 432 g Ba(NO3)2?</p><p>17. What is the number of moles of beryllium in 36 g of Be?</p><p>Percent Composition (use the molar mass to calculate the percent of the element)</p><p>18. What is the percent composition of chromium in BaCrO ?</p><p>19. What is the percent of carbon in acetone, C H O?</p><p>Chemistry CPA Final Exam Study Guide - 2014 7 Callahan, Pengitore & Ricafort Stoichiometry</p><p>MgCl2 + NaOH  Mg(OH)2 + NaCl</p><p>20. Balance the above reaction.</p><p>21. What is the mole ratio of MgCl2 to NaOH?</p><p>22. Identify the limiting reactant if 2 mole of MgCl2 and 2 mole of NaOH are used in a reaction.</p><p>Li + H(OH)  LiOH + H2</p><p>23. Balance the above reaction.</p><p>24. What is the mole ratio of Li to water?</p><p>25. Identify the limiting reactant if 2 mole Li and 2 mole of water are used in a reaction.</p><p>Lab Questions – Know/be able to do:</p><p> If you are given grams from lab data, convert to moles</p><p> How to determine the mole ratio from lab data (Moles of Fe and Cu lab)</p><p> Predict the products of a single-replacement reaction:</p><p> o Mg + HCl  ______+ ______?</p><p>8 Chemistry CPA Final Exam Study Guide - 2014 9 Callahan, Pengitore & Ricafort Unit 7: Solution Chemistry</p><p>26. Given grams how do you solve for moles? Example: convert 90 grams of water to moles.</p><p>27. Molarity is equal to __.</p><p> a. Grams of solute / moles of solute</p><p> b. Volume of solution x moles of solute</p><p> c. Moles of solute / liters of solution </p><p> d. Volume of solution / grams of solute</p><p>28. What mass of methanol, CH3OH, must be dissolved to make 1.50 L of a 0.675M solution? SHOW YOUR WORK!!!!</p><p>29. What is the molarity of a solution of HNO3 that contains 250 grams HNO3 in 3 L of solution? Convert grams to moles first.</p><p>30. What volume of 18.0 M H2SO4 is needed to contain 200 g H2SO4? Convert grams to moles first.</p><p>10</p><p>31. How many moles of CaCl2 are required to prepare 2.00 liters of 0.700 M CaCl2?</p><p>32. How many grams of NaI would be used to produce a 2.0 M solution with a volume of 1.0L? Solve for moles and convert your answer to grams.</p><p>Chemistry CPA Final Exam Study Guide - 2014 11 Callahan, Pengitore & Ricafort Use this solubility curve to answer the next set of questions (#33- 37) on the following page:</p><p>12 o 33. If there are 100 grams of KNO3 dissolved in 100 g of water at 70 C, the solution is __. a. saturated b. unsaturated c. supersaturated</p><p> o 34. If there are 10 grams of NaCl dissolved in 100 g of water at 30 C, the solution is __. a. saturated b. unsaturated c. supersaturated</p><p>35. If there are 70 grams of KBr dissolved in 100 g of water at 20oC, the solution is __. a. saturated b. unsaturated c. supersaturated</p><p> o 36. If there are 120 grams of NaClO3dissolved in 100 g of water at 60 C, the solution is __. a. saturated b. unsaturated c. supersaturated</p><p> o 37. If there are 190 grams of KNO3 dissolved in 100 g of water at 70 C, the solution is __. a. saturated b. unsaturated c. supersaturated</p><p>Chemistry CPA Final Exam Study Guide - 2014 13 Callahan, Pengitore & Ricafort Lab Questions: Know/be able to do:</p><p> What “like dissolves like” means</p><p> Polar dissolves polar and nonpolar dissolves nonpolar</p><p> polar and nonpolar do not dissolve</p><p> water is a polar molecule and makes hydrogen bonds</p><p>14 Unit 8: Gas Laws and KMT</p><p>Kinetic Molecular Theory and Heating Curves</p><p>38. What is the kinetic molecular theory?</p><p>39. How are temperature and kinetic energy related? </p><p>40. When a substance is in a single state of matter and the temperature is increasing, there will be an increase in the (kinetic energy/potential energy) of the particles.</p><p>41. When a substance is undergoing a phase change and the temperature is not changing, there will be an increase in the (kinetic energy/potential energy) of the particles.</p><p>Chemistry CPA Final Exam Study Guide - 2014 15 Callahan, Pengitore & Ricafort For questions 42 – 45, use the following graph: </p><p>42. What is the melting point of: a. substance A? b. substance B?</p><p>43. Which substance will melt first?</p><p>44. What is the boiling point of: a. substance A? b. substance B?</p><p>45. Which substance will boil first?</p><p>16 The Gas Laws Gas Law Theory</p><p>46. Draw and label the graph for each gas law (Boyle’s, Charles’, Gay- Lussac).</p><p>47. Why is it easier to compress a gas than it is to compress liquids or solids?</p><p>48. Why does air escape a tire valve when the cap is removed? </p><p>49. Is atmospheric pressure the highest below, at, or very high above sea level? </p><p>Chemistry CPA Final Exam Study Guide - 2014 17 Callahan, Pengitore & Ricafort Gas Law Calculations</p><p>50. A 500.0 mL sample of gas is collected at 745.0 torr. What will the volume be at 760 torr? Gas Law: ______</p><p>51. A 2L sample of gas at 100 K is heated to 150 K. What is the new volume? Gas Law: ______</p><p>52. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and then I raise the pressure to 14 atm, what is the new volume of the gas? Gas Law: ______</p><p>53. A gas takes up a volume of 17 liters, and a temperature of 299 K. If I raise the temperature to 350 K what is the new volume of the gas? Gas Law: ______</p><p>18 54. I have a gas at a volume of 0.5 L and a temperature of 325 K. If I raise the volume to 1.2 L, what will be the new temperature? Gas Law: ______</p><p>55. If I have 21 liters of gas at a temperature of 900 K, what will be the volume of the gas if I decrease the temperature to 750 K? Gas Law: ______</p><p>56. If I have a sample of gas at 300 K and a pressure of 5 atm, what will be the temperature of the gas if I decrease the pressure to 3 atm? Gas Law: ______</p><p>57. A gas occupies a fixed volume at 285 K at 1 atm. If the pressure increases to 3 atm, what is the new temperature? Gas Law: ______</p><p>Chemistry CPA Final Exam Study Guide - 2014 19 Callahan, Pengitore & Ricafort 58. A sample of nitrogen gas (N2) occupies a volume of 0.25 L at a pressure of 2 atm and 22°C. How many moles of N2 gas are there in this sample? Gas Law:______</p><p>59. How many grams of N2 gas are there in question 66? (Hint: use moles to grams conversion!)</p><p>60. A 4.5 mole sample of gas occupies a volume of 1.3 L at a temperature of 293 K. What is the pressure of the gas? Gas Law:______</p><p>20 Unit 9: Acids & Bases</p><p>61. List the properties for acids below.</p><p>62. List the properties for bases below.</p><p>63. What happens when an acid is mixed with a base? (Write the general form for the reaction that happens)</p><p>64. What is the range of the pH scale?</p><p>65. What is the pH range for acids?</p><p>66. What is the pH range for bases?</p><p>67. What is the pH for a neutral solution?</p><p>Chemistry CPA Final Exam Study Guide - 2014 21 Callahan, Pengitore & Ricafort 68. pH + pOH = </p><p>69. Complete the chart </p><p>[H+] pH [OH-] pOH Acid , Base, Neutral</p><p>11</p><p>7</p><p>1 x 10-2</p><p>1 x 10-2</p><p>22 70. Review the sample data table below from a student’s lab and answer the following questions. </p><p>Test Property</p><p>Test Solutions</p><p>A B C</p><p>Conductivity Very strong Very strong none</p><p>Litmus Paper Turns Red Turns Blue No change</p><p>Phenolphthalein colorless Pink color change colorless</p><p> pH Test Paper</p><p>4.0 10.0 7.0</p><p>Universal Indicator</p><p>Red Purple Green</p><p>Reaction with Magnesium</p><p>Produces a gas none none</p><p>Chemistry CPA Final Exam Study Guide - 2014 23 Callahan, Pengitore & Ricafort Questions to go with the #62 Data Table: </p><p>A. Is Solution A an acid, base, or neutral? Why?</p><p>B. Is Solution B an acid, base, or neutral? Why?</p><p>C. Is Solution C an acid, base, or neutral? Why?</p><p>D. What are the chemical properties that this student tested?</p><p>E. What are the physical properties that this student tested? </p><p>F. What were the qualitative observations this student made?</p><p>G. What are the quantitative observations this student made?</p><p>24</p>