Chemistry Spring 2018 Final Exam Review

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1 Name Date Period Chemistry Spring 2018 Final Exam Review TURN THIS COMPLETED REVIEW IN TO YOUR TEACHER BY DAY OF YOUR FINAL FOR A 5 point FINAL EXAM BONUS Unit #7 Moles 1. What is a mole? 2. What is molar mass? 3. What are the 3 types of representative particles? Use the conversion guide: MASS (g) MOLES PARTICLES 1 mol molar mass(g) 6.02 x particles 1 mole 4. Calculate the molar mass of Ca3(PO4)2. 5. How many moles are in 3.54 grams H2S? 6. How many grams are in 1.97 moles of carbon dioxide? 7. How many atoms are in 700 g of lithium? 8. How many molecules are in 0.42 moles of C3H8? Unit 8 Reactions 9. What element can tin replace during a single replacement reaction? Lithium, Magnesium, or Lead. 10. Will the following single replacement reactions occur? Yes or No? IF YES, write the products below. BaF 2 + Cl 2 ( Y / N ) Na + CuCl 2 ( Y / N ) Au + KF ( Y / N ) Cl 2 + LiBr 2 ( Y / N )

2 11. Fluorine gas (F2) is bubbled through a solution of sodium chloride (NaCl). What are the products formed in this reaction? 12. Are the following compounds soluble (aq) or insoluble (s) in water? MgCl 2 Na 2SO 4 AlPO 4 CaCO Will the following double replacement reactions occur? Yes or No? IF YES, write the products to the right. BaBr 2 + NaClO 3 ( Y / N ) CaS + KNO 3 ( Y / N ) Ag 2SO 4 + CuI 2 ( Y / N ) BaCO 3 + CaO ( Y / N ) 14. In a balanced chemical reaction the following symbols have important meanings (s) means (g) means (l) means (aq) means (dissolved in ) 15. Balance the following equations and label what kind of reaction it is, and check the Redox box if the reaction is considered a Redox reaction: (Synthesis, Decomposition, Single Replacement, Precipitation, Acid Base (Neutralization), Combustion) Li 2CO 3 + BaBr 2 LiBr + BaCO 3 C 10H 8 + O 2 CO 2 + H 2O Ca(OH) 2 + H 3PO 4 Ca 3(PO 4) 2 + H 2O B + F 2 BF 3 REDOX REDOX REDOX REDOX HI H 2 + I 2 REDOX K + Zn(NO 3) 2 Zn + KNO 3 REDOX 16. For the following redox reactions label the charge of all the elements in the reaction: 2 Mg + O 2 2 MgO Al + FeO Al 2O 3 + Fe Unit 9 Stoichiometry 17. The calculation of quantities in chemical equations is called. 18. In every chemical reaction, what values are always conserved? and. 19. The laws of conservation of mass states that the mass of the reactants always. 20. According to the law of conservation of mass if 9 atoms of hydrogen react with 3 atoms of carbon, how many atoms of hydrogen and atoms of carbon should be on the product side of the reaction?

3 21. Complete the following mole ratios 4 C4H8 + 6 O2 4 CO2 + 4 H2O C4H8 O2 O2 C4H8 C4H8 O2 CO2 H2O CO2 H2O 22. What is a limiting reactant? 23. What is an excess reactant? 24. How many moles of Ca are need to completely react 3.5 moles Al 2O 3? 3 Ca + Al 2O 3 3 CaO + 2 Al For questions 17-19, use the following reaction: 1 Ba(NO 3) Li 2O 1 BaO + 2 LiNO Calculate the number of moles of BaO that are produced when excess Ba(NO 3) 2 reacts with 5.5 mol of LiNO If you are given 100 grams of Li 2O, how many grams of LiNO 3 can theoretically be produced? 27. In a lab investigation, 421 g of lithium nitrate were synthesized by a group of students. Before starting the investigation, the students calculated that they should generate g of lithium nitrate. What is the actual yield? What is the theoretical yield? What is the percent yield of their investigation?

4 Unit 10 Gases Kinetic/Molecular Theory Circle TRUE/FALSE for each statement below 28. ( T / F ) Gas particles in a closed container attract and repel each other strongly. 29. ( T / F ) Gas particles are far apart from each other. 30. ( T / F ) Gas particles are larger than the distances in between the particles. (This explains high compressibility.) 31. ( T / F ) Compressibility means that gases can be compressed because they are far apart from each other. 32. ( T / F ) All gas particles move in constant, random motion. 33. ( T / F ) When gas particles collide, no kinetic energy is lost (collisions are perfectly elastic) C = K 300 K = C mole of ANY gas at STP = L 1 mole of any gas = particles 36. Pressure and volume have a/an relationship. When pressure increases, volume. 37. Pressure and temperature have a/an relationship. When pressure decreases, temperature. 38. Temperature and volume have a/an relationship. When temperature increases, volume. 39. When temperature increases, kinetic energy. 40. What causes pressure to increase?. 41. A container with an initial volume of 20 L is occupied by a gas at a pressure of 150 kpa and a temperature of 15 C. By changing the volume of the container the pressure of the gas increases to 450 kpa as the temperature is raised to 95 C. What is the new volume of the gas? 42. An 8.4L sample of O 2(g) at 1.9 atm has a moles. What is the Kelvin temperature of the sample? 43. A mixture of gases at a total pressure of 810 mmhg contains N2, CO2 and O2. The partial pressure of CO2 is 290 mmhg and the partial pressure of N2 is 270 mmhg, what is the partial pressure of the O2?

5 Unit 11 Chemical Bonding 44. Group 17, which has valence electrons, is called the. 45. Group 18 are called the 46. At room temperature ionic compounds can be( SOLIDS / LIQUIDS / GASES / ALL OF THE ABOVE ) 47. At room temperature covalent compounds can be( SOLIDS / LIQUIDS / GASES / ALL OF THE ABOVE ). 48. List 3 properties of ionic compounds 49. List 3 properties of covalent compounds 50. Complete the following table Compound Ionic or Covalent Bonds Dissolve in water High/Low Melting Point Conducts Electricity in solution NaBr NO 2 CH 4 FeCl The states that elements are most stable with 8 valence electrons. Which element is the main exception to the Octet Rule? Why? 52. The VSEPR theory states that molecules arrange themselves so that their are as far apart as possible. 53. List the 7 diatomic elements. Chemical Formula Lewis Dot Structure Draw in box Electron Pair Geometry example: linear # Of Lone Pairs on Central Atom SiH4 OBr2 PF3

6 Solubility (grams solute in 100mL H 2 O) Unit 12 - Solutions 54. In a solution of saltwater, is the solute and is the solvent. 55. What 3 factors affect solubility (or how MUCH will dissolve)? Label the one that is only applicable to gases What 3 factors affect rate of solubility (or how FAST a solute will dissolve)? Saturation curves: NaNO KBr KNO NaCl Temperature ( C) a) What mass of NaCl will dissolve in 100ml of H 2O at 10 C? b) If 130 grams of KNO 3 are dissolved in 100mL of 50 C water, is the solution saturated, unsaturated, or supersaturated? c) If 20 grams of NaCl are dissolved in 100mL of 80 C water, is the solution saturated, unsaturated, or supersaturated? d) How much KBr will diisolve in 25 ml of water at 10 C? 58. Miscible means that two liquids dissolve into each other. 59. Immiscible means that they dissolve into each other. 60. A dilute solution contains a amount of solute; 61. A concentrated solution contains a amount of solute.

7 62. Complete the table and answer the questions: Solution Moles of NaCl Volume of Water Concentration A 2 2 L B 4 3 L C 6 7 L a. Which solution above is the most concentrated? b. Which solutions above is the most diluted? 63. solutions contain the maximum amount of solute that can be dissolved at a particular temperature. 64. solutions contain less than the maximum; (more could be dissolved) 65. solutions contain more than the maximum; (too much is dissolved achieved by saturating a solution, then cooling the solution. Only temporary) 66. What kind of substances are always electrolytes (Conduct Electricity)? 67. Give four different examples of electrolytes: 68. What is the molarity of 2.5 L of solution that contains 2.0 mol MgCl 2? 69. If you dilute70.0 ml of 5.0 M NaCl to make a ml of solution, what is the molarity of the dilute solution?

8 Unit 13 Acids and Bases 70. List 5 properties of acids. 71. List 5 properties of bases. 72. A solution with a ph and poh of 7 is considered to be. 73. Name the following Acids c. HCl d. HBr e. H 3P f. HClO 2 g. H 2SO 4 h. H 3PO Which bases are considered strong? 75. Label the following as strong acid (SA), weak acid (WA), strong base (SB), or weak base (WB): HBr Fe(OH) KOH Be(OH) 2 Al(OH) 3 H 3PO 3 Li(OH) HNO3 Ca(OH) What is a B-L acid? a B-L base? 77. In the equation below, label the B-L acid, B-L base, conjugate acid, and conjugate base. H 2S + H 2O HS - + H 3O + _ NH 3 (aq) + H 2O (l) NH 4 + (aq) + OH - (aq) 78. H 3P is a Brønsted-Lowry Acid. What is its conjugate base? 79. H 2SO 4 is a Brønsted-Lowry Acid. What is its conjugate base? 80. Identify the Arrhenius acid (AA) or base (AB) KOH H 3PO 4 HF Cu(OH) 2 HCl NaOH H 2CO 3 NH 4OH

9 81. Complete the following neutralization reactions: i. LiOH + H 2CO 3 j. H 3PO 4 + Ca(OH) Answer the questions using the following chart: Solution ph Solution ph Solution Solution Solution Solution a) Which solution is the most acidic? b) Which solution has the greatest [H + ]? c) Which solution is the most basic? d) Which solution has the greatest [H + ]? 83. Fill in the blanks in the below table. [H+] ph poh Acid/Base/Neutral 4.21 x 10-5 M 1.0 x M 1.0 x 10-7 M 84. What volume of M Ca(OH) 2 is neutralized by ml of M HBr? 2 HBr + 1 Ca(OH) 2 2H 2O + 1 CaBr 2

10 Unit 14 Thermochemistry 85. Fill in the Chart Process Heat absorbed or released? ΔH Sign? What do you feel? Heat shows up as reactant or product? Which has higher PE: Reactants or Products? Exothermic Endothermic 86. Pick Endothermic or Exothermic a. Heat is a reactant b. Energy is absorbed c. Energy is a product d. Heat is released e. A + B + Heat C + D f. A + B + C + D Heat g. In a reaction the beaker feels warmer h. In a reaction the beaker feels colder 87. Use the energy diagram to answer the following questions. a) What is the potential energy of the reactants in kj? b) What is the potential energy of the products in kj? c) What is the ΔH in kj? d) Is this reaction endothermic or exothermic? e) Was energy absorbed or released during the reaction? 88. What is the ΔH for the following Reactions: a. CaO(s) + H2O(l) Ca(OH)2 (s) kj endothermic/exothermic heat released/absorbed ΔHrxn b. 2 CO (g) + O2 (g) kj 2 CO2 (g) endothermic/exothermic heat released/absorbed ΔHrxn 89. Rewrite the following equations by expressing the energy change as a term in the equation: a) H2O (g) H2O (l) ΔH = kj b) 2 H2SO4 2 SO2 + 2 H2O + O2 ΔH = kj 90. Given the reaction below, how much energy would be released if 3 moles of H2O were used? CaO(s) + H2O(l) Ca(OH)2 (s) kj ΔH

11 91. Calculate the amount of energy produced when 60 grams of oxygen combust with ethanol. C2H5OH + 3O2 2CO2 + 3H2O kJ ΔH = Joules are used to heat water from 23.0 C to 67.0 C. What is the mass of the water? The specific heat of water is J/g- C 93. When 435 J of heat is added to 3.4 g of olive oil at 21 C, the temperature increases to 85 C. What is the specific heat of olive oil? 94. Predict whether the following reaction will be spontaneous at 325K by calculating G o from the given enthalpies and entropies. G o = H - T S NH4Cl (s) NH3 (g) + HCl (g) H o = +176 kj/mol and S o = kj/(mol*k) 95. Predict whether the value of S for each of the following reactions will greater than, less than, or equal to zero. C3H7CO2H(s) + 4O2(g) 3 CO2(g) + 4 H2O(g) 3O2 (g) + P2 (g) 2 PO3 (g) H2O (s) H2O(l) 2Ca (s) + Cl2 (g) -> 2 CaCl2 (s) 96. Match the example to the type of heat transfer Convection Conduction Convection a. Beaker sitting on hotplate b. Hot air rising c. Warmth felt at distance to side of hot plate

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided