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Name______________________________________ Period _________ AP Chemistry Midterm I Review 1. Indicate the number of significant figures for each number: a. 354 ____ b. 0.00809 ____ c. 4,000 ____ d. 5,000,300 ____ 5 f. 6.75 x 10 ____ 32 g. 9.9000 x 10 ____ h. 0.00000008 ____ e. 600.0 ____ i. 0.7702 ____ 2. Make the following calculations and give your final answers with correct number of sig figs. a. 7.992 4.67 + 12.887 b. 9.66 -7 c. 4.44 x 2.1_ d. 824.8 ÷ 2 e. 9.83 - 7.0 f. 2.35 +80.9 3. Determine if each situation is accurate, precise, both, or neither. a. After 4 trials, Seth determined that the density of water was 1.0g/mL, 1.1 g/mL, .9 g/mL and 1.0 g/mL b. After 4 trials, Aidan determined that the density of water was 2.0 g/mL, 2.5 g/mL, 1.98 g/mL and 1.0 g/mL c. After 4 trials, Sheldon determined that the density of water was 2.5g/mL, 2.6 g/mL, 2.56 g/mL and 2.45 g/mL 4. Put the following into proper scientific notation. a. 40,000 __________________ c. 567 __________________ b. 0.0065 __________________ d. 0.0002022 __________________ e. 20,000,000 __________________ f. 23,000 __________________ g. 92.3 h. 210,000 __________________ __________________ 5. DENSITY – Show all work. Don’t forget units and sig figs!!!!! Circle your final answer. a. What is the density of a piece of wood that has a mass of 25.0 grams and a volume of 29.4 cm3? b. You have a box filled with 15 vials of aqueous sodium chloride. The total mass of the sodium chloride is 52.5g and each vial holds 3.2 mL of the solution. What is the density of the solution in kg/L? c. An ice cube measuring 5.80 cm by 5.80 cm by 5.80 cm has a density of 0.917 g/mL. What is the mass? 6. Identify each of the following as an element (E), compound (C), or mixture (M). ______soil ______kool-aid ______paper ______copper ______sulfur ______baking soda, (sodium ______milk ______helium hydrogen carbonate) ______carbon dioxide _____mercury ______sugar ______water Name______________________________________ Period _________ 7. Which from #6 would be considered pure substances? 8. List the signs of a chemical change 9. Why are the changes -heat released and color change- not considered chemical changes unless accompanied by another sign of a chemical reaction? 10. Identify each mixture below as homogeneous or heterogeneous mixtures. _______________ chocolate chip cookie _______________ river water _______________ cough syrup _______________ salt water solution _______________ steel _______________ pure air _______________ Diet Coke _______________ granite 11. Identify the described properties as Physical (P) or Chemical (C). _______ odorless _______ mass of 5.00 grams _______ tarnishes rapidly in air _______ boiling point of 883 C _______ soft, silver-white _______ reacts violently with water _______ reacts with acid 12. Indicate Physical (P) or Chemical (C) change for each example. ________ Metal is heated until it turns red. ________ Aluminum & oxygen react to produce aluminum oxide. ________ An iron nail rusts. ________ Copper metal is hammered into a thin sheet. ________ An ice cube melts. ________ Magnesium chloride is dissolved in water. ________ Hydrochloric acid neutralizes sodium hydroxide to form sodium chloride and water. 13. Why are phase changes considered only physical changes? 14. Sketch an example of the following at the molecular level: a. a gaseous compound b. a mixture of elements that is a solid c. a gaseous mixture of elements and compounds 15. What is the percentage of sodium (by mass) in sodium phosphate? (42.1%) 16. For the hydrate sodium sulfate decahydrate, calculate the following: (a) the percent of sodium (by mass) in the hydrate (14.3%) (b) percent of TOTAL oxygen (by mass) in the hydrated compound. (69.6%) (c) Percent of water (by mass) in the hydrate (55.9%) 17. Calculate the percentage of nitrogen (by mass) in the ammonium nitride (82.4%) 18. Find the empirical formula for a compound that contains 32.8 g chromium and 67.2 g chlorine.(CrCl3) 19. The hydrocarbon used in the manufacture of foam plastics is called styrene. Styrene contains 92.25% carbon and 7.75% hydrogen. What is the empirical formula of styrene? If the molar mass of styrene is 104 g/mol, what is the molecular formula? 20. Phenanthrene is a hydrocarbon, a compound consisting only of C and H. If you burn 0.215 g of the compound, and find that it produces 0.747 g of CO2 and 0.109 g of H2O, determine the empirical formula of the compound. 21. How many moles are there in 768 grams of iron (III) sulfate?(1.92 mol) 22. How many moles are there in 1200g of potassium dichromate?(4.1 mol) 23. You have 13.2 moles of lead (II) nitrate. How many grams is this? (4.37 x 103 g) 24. How many moles are there in 78 grams of nitrogen gas?(2.8 mol) 25. NAME THE FOLLOWING COMPOUNDS: 1. BaSO3 14. AgNO3 2. (NH4)3PO4 15. As2O5 3. PBr5 16. Fe2O3 4. MgSO4 17. HClO 5. CaO 18. N2O3 6. H3PO4 19. HF 7. Na2Cr2O7 20. H2C2O4 8. MgO 21. NaHCO3 9. SO3 22. SiBr4 10. Cu(NO3)2 23. CuCl2 11. HI 24. HNO2 12. N2O 25. SnO2 13. MnO 26. BaCrO4 WRITE FORMULAS FOR THE FOLLOWING COMPOUNDS: 27. hydrobromic acid 40. diphosphorus pentoxide 28. chromium(III) carbonate 41. sulfurous acid 29. magnesium sulfide 42. lead(II) nitrate 30. iodine trichloride 43. dihydrogen monoxide 31. lithium hydride 44. sodium oxalate 32. ammonium hydroxide 45. perchloric acid 33. calcium chloride 46. chlorous acid 34. hydroselenic acid 47. silicon dioxide 35. iron(II) nitride 48. carbonic acid 36. aluminum hydroxide 49. sodium chlorate 37. tin(II) fluoride 50. xenon hexafluoride 38. sulfur tetrachloride 51. nickel nitrate 39. mercury(II) iodide 52. potassium perchlorate 26. Calcium nitrate can be produced by reacting excess nitric acid with calcium hydroxide. a. If 7.40g of calcium hydroxide reacts with excess nitric acid, how many grams of calcium nitrate are formed?(16.4grams) b. If you performed the same reaction above in the lab and obtained 14.3g of calcium nitrate, what is your percent yield? c. How many grams of nitric acid are needed for a complete reaction (all 7.40 g of calcium hydroxide are consumed) Write the net ionic equation for the following: 27. Solutions of lead (II) nitrate and lithium chloride are mixed (Pb2+ + 2Cl- → PbCl2) 28. Solutions of silver acetate and barium chloride are mixed (Ag+ + Cl- → AgCl) 29. Solutions of tin (II) fluoride and lithium carbonate are mixed. (Sn2+ + CO32- → SnCO3) 30. Solid sodium bicarbonate is mixed with a concentrated solution of acetic acid (NaHCO3 + HC2H3O2 → Na+ + C2H3O2- + H2O + CO2) 31. Hydrochloric acid is mixed with a solution of sodium hydroxide (H+ + OH- → HOH) 32. Ammonia is added to water (NH3 + H2O ↔ NH4+ + OH-) 33. What is the equilibrium expression (Keq) dependent upon? 34. If the equilibrium constant for A + B 2C 2A + 2B is___________. C is 0.56, then the equilibrium constant for 35. If the concentration of the product were to double, what would happen to the equilibrium constant? 36. For the reaction H2(g) + Cl2(g) 2HCl(g), Kc = 1.22 x 1033 at a temperature of 301 K. What is Kp at this temperature? (1.22x 1033) 37. Consider the reaction What is the At 1273 K, the Kp value is 167.5. at equilibrium if the is 0.17 atm at this temperature? (5.3atm) 38. Consider the following reaction: 2HF(g) H2(g) + F2(g) (K = 1.00 10–2) Given 1.00 mole of HF(g), 0.362 mole of H2(g), and 0.750 mole of F2(g) are mixed in a 5.00 L flask, determine the reaction quotient, Q. (Q = 0.272) 39. Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Cl2(g) S2Cl2(g) + CCl4(g) When 2.14 mol of CS2 and 5.85 mol of Cl2 are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.620 mol of CCl4. How many moles of Cl2 are present at equilibrium? (3.99 mol) 40. Given the equation 2A(g) 2B(g) + C(g). At a particular temperature, K = 1.6 x 104. If you mixed 5.0 mol B, 0.10 mol C, and 0.0010 mol A in a one-liter container, which direction would the reaction initially proceed? (to the left) 41. Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and is allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g) If at equilibrium the N2O4 is 37% dissociated, what is the value of the equilibrium constant, Kc, for the reaction under these conditions? (0.87) 42. Consider the following system at equilibrium: N2(g) + 3H2(g) 2NH3(g) + 92.94 kJ Which of the following changes will shift the equilibrium to the right? (II, IV, V, VIII) I. increasing the temperature II. decreasing the temperature III. increasing the volume IV. decreasing the volume V. removing some NH3 VI. adding some NH3 VII. removing some N2 VIII. adding some N2 43. Consider the reaction, which is exothermic as written, PCl5 3(g) + Cl2(g). Which of the following changes would result in the production of MORE Cl2(g)? (II, VI, VII, VIII) I. II. III. IV. V. VI. VII. VIII. IX. adding PCl3(g) removing PCl3(g) reducing the volume of the container removing PCl5(g) increasing the temperature increasing the volume of the container adding PCl5(g) reducing the temperature adding a suitable catalyst 44. Given the equation 2A(g) 2B(g) + C(g). At a particular temperature, K = 1.6 x 104. At a higher temperature, K = 1.8 x 10–5. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will shift the reaction to the _______________. 45. A 50.0-mL sample of 0.10 M HNO2 (Ka = 4.0 x 10–4) is titrated with 0.12 M NaOH. The pH after 25.0 mL of NaOH have been added is________. (3.57) 46. For nitrous acid, HNO2, Ka = 4.0 x 10–4. Calculate the pH of 0.27 M HNO2. (1.98) 47. Which of the following is the correct order for increasing pHs for equimolar solutions of HNO3, KCl, NH4Cl, KOH, and NaC2H3O2? (Ka for HC2H3O2 is 1.80 x 10–5, Ka for NH4+ is 5.56 x 10–10). (HNO3, NH4Cl, KCl, NaC2H3O2, KOH) 48. The following question refers to a solution that contains 1.59 M hydrofluoric acid, HF (Ka = 7.2 x 10–4), and 3.00 M hydrocyanic acid, HCN (Ka = 6.2 x 10–10). What is the pH of this mixture of weak acids? (1.47) NOMENCLATURE REVIEW ANSWER KEY 1. barium sulfite 2. ammonium phosphate 3. phosphorus pentabromide 4. magnesium sulfate 5. calcium oxide 6. phosphoric acid 7. sodium dichromate 8. magnesium oxide 9. sulfur trioxide 10. copper(II) nitrate 11. hydroiodic acid 12. dinitrogen monoxide 13. manganese(II) oxide 14. silver nitrate 15. diarsenic pentoxide 16. iron(III) oxide 17. hypochlorous acid 18. dinitrogen trioxide 27. HBr 28. Cr2(CO3)3 29. MgS 30. ICl3 31. LiH 32. NH4OH 33. CaCl2 34. H2Se 35. Fe3N2 36. Al(OH)3 37. SnF2 38. SCl4 39. HgI2 40. P2O5 41. H2SO3 42. Pb(NO3)2 43. H2O 44. Na2C2O4 19. hydrofluoric acid 20. oxalic acid 21. sodium bicarbonate 22. silicon tetrabromide 23. copper(II) chloride 24. nitrous acid 25. tin(IV) oxide 26. barium chromate 45. HClO4 46. HClO2 47. SiO2 48. H2CO3 49. NaClO3 50. XeF6 51. Ni(NO3)2 52. KClO4