CHM130/Practice/Measurement

Transcription

1 CHM130/Practice/Measurement Name: 1. For each of the following, write the scale reading and identify the number of significant figures. Reading Number of significant figures 1

2 2. For each of the volume devices below record the scale reading. scale reading uncertainty scale reading uncertainty scale reading uncertainty

3 CHM130/Practice Significant Figures/Scientific Notations/Units/Prefixes Name: 1. Identify the number of significant figures in each of the following. a) cm b) 1090 ml c) g d) km e) 100. L f) in g) x g h) ml 2. Round off each of the following measurements to the number of significant figures (digits) given in the parenthesis. a) km (4) b) g (3) c) mm (3) d) ml (2) e) (3) 3. Write each of the following numbers in scientific notation. a) b) c) d) Complete the table. prefix symbol Numerical value c deci 1,000,000 µ kilo

4 5. Complete the table using the example given. Abreviation Full name Type of measurement m meter length ml kg cc nm dl 6. Complete the following relationship. a) 1 m = mm b) 1 L = dl c) 1 kg = g d) 1 g = µg e) 1 in = cm f) 1 lb. = g g) 1 m = cm h) 1 L = ml 4

5 CHM130 Practice (Measurements/Significant Figures in Calculations) Name: 1. Measure the length of a pencil in cm and mm with correct number of significant figures. mm cm 2. Give the answers for the following calculations with the proper number of significant figures. a) = b) x 3.02 = c) = d) = e) = e) (2.31 x 10 3 ) x (3.0 x 10 5 ) = f) 9.32 x x = g) x x = h) (4.122 x 10-5 ) x (1.76 x ) = i) (6.34 x ) x (3.325 x ) = 5

6 CHM130/Practice /Unit Equations/Conversion factors/factor-label Method Name: 1. Complete the unit equation and write two corresponding conversion factors for each of the following in the table. Unit equation 1 km = _1000_ m 1 cm = m Conversion factors 1 km 1000 m or 1000 m 1 km 1 g = mg 1 L = dl 1 cc = 1 ml 2. Use the appropriate conversion factor to solve the following problems by factor-label method (dimensional analysis method). Show your work. a) 26.5 mg = g b) cm = m c) 1.25 km = m d) 25.8 dl = L 6

7 CHM130/Practice/Factor-Label Method Name: Perform the following conversions by factor-label methods. example) Convert 1250 g to lb. i) plan: identify the given unit (g) and wanted value (lb) : g lb equality: find the unit relationship(s): 1 lb = 454 g two conversion factors from equality: 1lb 454 g or 454 g 1lb i problem-solving: use the appropriate conversion factor from to cancel the given unit and to obtain the wanted unit g x 1lb 454 g = 2.75 lb a) 76.3 L to dl i) plan: equality: two conversion factors: i problem-solving: b) mm to m i) plan: equality: two conversion factors: i problem-solving: 7

8 CHM130/Practice/Factor-Label Method Name: Perform the following conversions by factor-label methods. a) 175 lbs to kg (1 lb = 454 g) i) plan: conversion factors: i problem-solving: b) qt to L (4qts = 1 gal, 1 gal = L) i) plan: conversion factors: i problem-solving: c) µm to cm i) plan: conversion factors i problem-solving 8

9 CHM130/Practice/Temperature Conversions/Density Name: 1. Perform the following conversions. a) 78.0 o F to o C b) 105 o C to o F c) 34.5 o C to K d) 290 K to o C e) 372 K to o F f) 98.6 o F to K 2. A metal has a density of 11.2 g/cm 3. a) What would be the volume (in cm 3 ) of 96.5 g of the metal? b) How many grams would the metal with the volume of 46.5 cm 3 weigh? 9

10 CHM130/Practice/Percent as Conversion Factors Name: Show your work for the following problems. 1. A solution contains 23.5 grams of sugar and grams of water. a) Calculate the % sugar by weight. % sugar b) Write the conversion factors that can be obtained from the answer in a). c) How many grams of this solution would contain 12.8 grams of sugar? Solve this problem by factor-label method. g solution 2. A drink contains 4.5 % of real fruit juice by volume. How many ml of real fruit juice is in 155 ml of a drink? i) plan: conversion factors: i solving problem: ml real fruit juice 10

11 CHM130/Practice/Factor-label Method Name: 1. A solution of ethanol was prepared by mixing 34.5 g of ethanol with 295 g of water. a) What is the percent of ethanol by mass in this solution? b) Write the conversion factors you can obtain from a). c) How many grams of ethanol are there if you take 35.0 g of this solution? Solve this by factor label method. 2. A solid bar that measures 10.0 cm x 12.5 cm x 12.5 cm weighs 3250 g. a) Calculate the density of the solid. b) Write the density obtained for a) as two conversion factor forms. c) What volume in cc will 25.5 g of the solid occupy? Solve this by factor label method. 11

12 CHM130/Practice/Conversion Factors/Factor-label method Name: 1. Write two conversion factors for each of the following statements. a) A car travels 55 miles per hour. b) Twenty five candies are in a bag. c) A medication is given at 3.50 mg/kg body weight. 2. Solve the following problems using conversion factors. a) A water bottle has a volume of 500. ml. What is the capacity of the water bottle in liters? b) The length of a pencil is 20.5 cm. How long is the pencil in meters? c) Convert g to mg. 12

13 CHM130/Practice/Matter Name: 1. Define Matter. 2. Identify three states of matter. i) i 3. Identify which of the following represents a compound. i) 4. Which of the following indicates chemical change? i) + + Explain why. 5. Name each of the following changes of states. a) solid to liquid b) liquid to solid c) liquid to gas d) gas to liquid e) solid to gas f) gas to solid 13

14 7. The following represents the liquid state of water (H 2 O). a) Which of the following diagrams best represents water (H 2 O) molecules after liquid water was heated to vaporize? i) i Is vaporization physical or chemical change? Explain your reasoning. b) Water (H 2 O) can be decomposed into hydrogen gas (H 2 ) and oxygen gas (O 2 ) by the process called electrolysis. Draw the diagram of hydrogen gas and oxygen gas. i) Electrolysis Is an electrolysis physical or chemical change? Explain your reasoning. 14

15 CHM130/Practice/Physical and Chemical Changes Name: 1. Classify each of the following as physical or chemical change. a) breaking glassware b) drying clothes c) burning wood d) digesting a cookie e) chopping an onion f) inflating a balloon g) dissolving an antacid tablet in water h) rusting iron metal 2. Classify each of the following as an element, compound, or mixture. a) air b) table salt (NaCl) c) copper d) bronze alloy e) ore 15

16 CHM130/Practice/Element/Atom Name: Write the symbols of the following elements. Name of Element symbol Name of Element symbol Hydrogen Lithium Potassium Magnesium Strontium Radium Manganese Cobalt Palladium Copper Gold Cadmium Boron Carbon Tin Nitrogen Arsenic Bismuth Sulfur Fluorine Bromine Neon Krypton Xenon Cesium Helium Sodium Beryllium Calcium Barium Chromium Iron Nickel Platinum Silver Zinc Mercury Aluminum Silicon Lead Phosphorus Antimony Oxygen Selenium Chlorine Iodine Argon Titanium Germanium Radium 16

17 CHM130/Practice/Element/Atom Name: Write the names of the following elements. symbol Name of Element symbol Name of Element Cu Li Pt Mg Sr Kr Ca Co Pd H Si C B Cd Sn Ti Ge Bi S F Br Ne Ra Cr O I Al Mn Ba Xe Fe Ni K Au Zn Hg Be Ag Pb P Sb He Se Cl Na Ar N As 17

18 CHM130 Practice (Atomic Structure) Name: 1. Complete the table by providing the missing information. Name of element Atomic notation Atomic number Mass number Number of protons Number of neutrons Number of electrons Sodium Al Potassium Lithium Ni 2. Describe an atom according to (a) the Dalton model, (b) the Thomson model, and (c) the Rutherford model. (a) The Dalton model (b) The Thomson model (c) The Rutherford model 18

19 CHM130 Extra (Electron Configuration) Name: 1. Write the electron configuration for each of the following and identify the valence shell and number of valence electrons. Element Electron configuration Valence shell # of valence electrons um on horus sium num mine 2. Classify each of the following element as metal, nonmetal, or metalloid. a) silicon b) silver c) aluminum d) chlorine e) cesium f) copper 3. Write the names of seven elements that exist as diatomic molecules. 19

20 CHM130 practice Name: Complete the table by writing formulas and names of the compounds. Cl - O 2- N 3- S 2- Na + Na 2 O Sodium oxide Cu + Ca 2+ Ni 2+ Fe 3+ Fe 2 S 3 Iron(III) sulfide Al 3+ 20

21 CHM130 Practice (Nomenclature) Name: 1. Write the names of the following compounds. a) Ni 2 S 3 b) HgO c) H 3 P (aq) d) CsF e) OF 2 f) ZnBr 2 g) Ag 2 O h) Cu 3 N i) S 2 F 10 j) H 2 S (aq) k) N 2 O 4 2. Write the formulas of the following compounds. a) Diphosphorus pentoxide b) Tin(II) fluoride c) Chromium(III) nitride d) Iodine trichloride e) Hydroselenic acid f) Calcium hydride g) Strontium sulfide 21

22 CHM130 Practice (Nomenclature) Name: 1. Name each of the following binary compounds. MgS K 3 N P 4 O 10 H 2 S (aq) NO Fe 2 S 3 H 2 Se (aq) PbBr 2 Hg 2 I 2 OCl 2 BeH 2 Sr 3 P 2 2. Write the formula for each compound. Silver hydride Cesium nitride Phosphorus tribromide Hydrobromic acid Copper(II) sulfide Barium fluoride Tin(IV) carbide 22

23 CHM 130 Practice (Nomenclature) Name: 1. Write correct formula for each of the following compounds. a) sodium bromide b) magnesium sulfide c) potassium nitride d) copper(i) oxide e) calcium phosphide f) dichlorine pentaoxide g) iron(iii) iodide h) lithium hydride 2. Name the following compounds. a) SO 2 b) NiCl 2 c) K 2 O d) CBr 4 e) AlN f) AgF g) Br 3 O 8 23

24 CHM130 Nomenclature (Binary Acids) Name: Write the names of the following acids. 1. HI (aq) 2. HCl (aq) 3. H 3 N (aq) 4. H 2 S (aq) 5. HF (aq) 6. H 2 Se (aq) 7. H 3 P (aq) Write the formulas of the following acids. 1. hydrobromic acid 2. hydrofluoric acid 3. hydrocarbonic acid 4. hydrosulfuric acid 5. hydronitric acid 6. hydrophosphoric acid 7. hydroarsenic acid 24

25 CHM130 Practice (Nomenclature/Acids) Write formulas for the following acids. 1. hydrochloric acid 2. perchloric acid 3. chloric acid 4. chlorous acid 5. hypochlorous acid 6. nitric acid 7. sulfuric acid 8. hydrosulfuric acid 9. nitrous acid 10. phosphoric acid 11. acetic acid 12. hydronitric acid 13. hydrofluoric acid 14. phosphorous acid 15. iodic acid Write names of the following acids. 16. HBr (aq) 17. HBrO (aq) 18. HBrO 2(aq) 19. HBrO 3(aq) 20. HBrO 4(aq) 21. H 3 P (aq) 22. H 2 SO 3(aq) 23. H 2 CrO 4(aq) 24. H 2 CO 3(aq) 25. HI (aq) 26. H 2 Se (aq) 27. H 3 PO 3(aq) 25

26 CHM130 Practice (Nomenclature/Acids) Write the names of the following acids. 1. HCl (aq) 2. HClO 4(aq) 3. HClO 3(aq) 4. HClO 2(aq) 5. HClO (aq) 6. HNO 3(aq) 7. H 2 SO 4(aq) 8. H 2 S (aq) 9. HNO 2(aq) 10. H 3 PO 4(aq) 11. HC 2 H 3 O 2(aq) 12. H 3 N (aq) 13. HF (aq) 14. H 3 PO 3(aq) 15. HIO 3(aq) Write the formulas of the following acids. 16. hydrobromic acid 17. hypobromous acid 18. bromous acid 19. bromic acid 20. perbromic acid 21. hydrophosphoric acid 22. sulfurous acid 23. chromic acid 24. carbonic acid 25. hydroiodic acid 26. hydroselenic acid 27. phosphorous acid 26

27 CHM130 Practice (Nomenclature) Name: 1. Complete the table by writing formulas and names of the compounds. Cl - OH - SO 4-2 PO 4-3 Na + Ca +2 Fe +3 NH Write the formula for each of the following compounds. a) Barium hydroxide b) Sulfuric acid c) Copper(I) phosphate d) Magnesium hydroxide e) Acetic acid 27

28 CHM130 Practice (Nomenclature) Name: Write the formulas for the following compounds. 1. lead (II) hydroxide 2. aluminum perchlorate 3. magnesium cyanide 4. lithium iodate 5. cobalt (III) nitrate 6. ammonium phosphate 7. dinitrogen pentoxide 8. sulfur hexabromide 9. barium sulfate 10. nickel (II) acetate 11. mercury (I) carbonate 12. antimony (III) chloride 13. cadmium phosphite 14. manganese (II) bicarbonate 15. nickel (II) fluoride 16. potassium dichromate 17. phosphorus pentabromide 18. copper (II) sulfite 19. calcium carbonate 20. copper(i) oxide 21. tin (IV) nitrate 22. iron (III) hydrogen sulfate 23. bismuth (III) nitrite 24. sulfur dioxide 25. dinitrogen trisulfide 28

29 26. tetraphosphorus decoxide 27. iodine monochloride 28. zinc acetate 29. iron (II) hydrogen sulfite 30. mercury (II) bromide 31. nickel (II) permanganate 32. barium oxide 33. tin (IV) cyanide 34. cobalt (II) chlorite 35. copper (I) sulfate 36. chromium (III) chloride 37. dichlorine heptoxide 38. silver dichromate 39. tin (II) chromate 40. strontium sulfite 41. potassium permanganate 42. iron (III) sulfate 43. mercury (I) sulfide 44. nickel (II) cyanide 45. dibromine momoxide 46. nitrogen trichloride 47. lithium phosphide 48. iodine monofluoride 49. carbon tetrabromide 50. iron (III) sulfite 29

30 CHM130 Practice (Nomenclature) Answer Key 1. lead (II) hydroxide Pb(OH) 2 2. aluminum perchlorate Al(ClO 4 ) 3 3. magnesium cyanide Mg(CN) 2 4. lithium iodate LiIO 3 5. cobalt (III) nitrate Co(NO 3 ) 3 6. ammonium phosphate (NH 4 ) 3PO 4 7. dinitrogen pentoxide N 2 O 5 8. sulfur hexabromide SBr 6 9. barium sulfate BaSO nickel (II) acetate Ni(C 2 H 3 O 2 ) mercury (I) carbonate Hg 2 CO antimony (III) chloride SbCl cadmium phosphite Cd 3 (PO 3 ) manganese (II) bicarbonate Mn(HCO 3 ) nickel (II) fluoride NiF potassium dichromate K 2 Cr 2 O phosphorus pentabromide PBr copper (II) sulfite CuSO calcium carbonate CaCO copper(i) oxide Cu 2 O 21. tin (IV) nitrate Sn(NO 3 ) iron (III) hydrogen sulfate Fe(HSO 4 ) bismuth (III) nitrite Bi(NO 2 ) sulfur dioxide SO dinitrogen trisulfide N 2 S tetraphosphorus decoxide P 4 O iodine monochloride ICl 28. zinc acetate Zn(C 2 H 3 O 2 ) iron (II) hydrogen sulfite Fe(HSO 3 ) mercury (II) bromide HgBr nickel (II) permanganate Ni(MnO 4 ) barium oxide BaO 33. tin (IV) cyanide Sn(CN) cobalt (II) chlorite Co(ClO 2 ) copper (I) sulfate Cu 2 SO chromium (III) chloride CrCl dichlorine heptoxide Cl 2 O silver dichromate Ag 2 Cr 2 O tin (II) chromate SnCrO strontium sulfite SrSO potassium permanganate KMnO iron (III) sulfate Fe 2 (SO 4 ) mercury (I) sulfide Hg 2 S 44. nickel (II) cyanide Ni(CN) dibromine monoxide Br 2 O 46. nitrogen trichloride NCl lithium phosphide Li 3 P 48. iodine monofluoride IF 49. carbon tetrabromide CBr iron (III) sulfite Fe 2 (SO 3 ) 3 30

31 CHM130 Practice (Nomenclature II) Write the names of the following compounds. Name: 1. PbI 2 2. Na 2 CO 3 3. Zn(HCO 3 ) 2 4. SnF 2 5. Al(ClO 3 ) 3 6. CF 4 7. PI 5 8. Al 2 O 3 9. Ag 2 CrO Pb(SO 3 ) (NH 4 ) 2 CO Fe(C 2 H 3 O 2 ) H 2 SO 4(aq) 14. Mg(MnO 4 ) Sr(ClO 4 ) Cl 2 S OF Cu(OH) Al(CN) CS HgS 22. P 4 S Ca(ClO 3 ) Cd(CN) KBrO Cr(HSO 4 ) Li 3 PO SnBr Hg 2 (NO 2 ) Ni 3 (PO 4 ) 2 31

32 31. K 2 O 32. Fe(ClO 2 ) Ca(HCO 3 ) CI PF Mn(ClO) BrCl Cr(NO 3 ) CoCO NCl BaSO CuClO 43. P 4 O Ni(C 2 H 3 O 2 ) 2 32

33 CHM130 Practice (Nomenclature II) Answer Key 1. PbI 2 lead (II) iodide 2. Na 2 CO 3 sodium carbonate 3. Zn(HCO 3 ) 2 zinc bicarbonate 4. SnF 2 tin (II) fluoride 5. Al(ClO 3 ) 3 aluminum chlorate 6. CF 4 carbon tetrafluoride 7. PI 5 phosphorus pentaiodide 8. Al 2 O 3 aluminum oxide 9. Ag 2 CrO 4 silver chromate 10. Pb(SO 3 ) 2 lead (IV) sulfite 11. (NH 4 ) 2 CO 3 ammonium carbonate 12. Fe(C 2 H 3 O 2 ) 3 iron (III) acetate 13. H 2 SO 4(aq) sulfuric acid 14. Mg(MnO 4 ) 2 magnesium permanganate 15. Sr(ClO 4 ) 2 strontium perchlorate 16. Cl 2 S 7 dichlorine heptasulfide 17. OF 2 oxygen difluoride 18. Cu(OH) 2 copper (II) hydroxide 19. Al(CN) 3 aluminum cyanide 20. CS 2 carbon disulfide 21. HgS mercury (II) sulfide 22. P 4 S 5 tetraphosphorus pentasulfide 23. Ca(ClO 3 ) 2 calcium chlorate 24. Cd(CN) 2 cadmium cyanide 25. KBrO 2 potassium bromite 26. Cr(HSO 4 ) 3 chromium (III) bisulfate 27. Li 3 PO 4 lithium phosphate 28. SnBr 4 tin (IV) bromide 29. Hg 2 (NO 2 ) 2 mercury (I) nitrite 30. Ni 3 (PO 4 ) 2 nickel (II) phosphate 31. K 2 O potassium oxide 32. Fe(ClO 2 ) 2 iron (II) chlorite 33. Ca(HCO 3 ) 2 calcium bicarbonate (or calcium hydrogen carbonate) 34. CI 4 carbon tetraiodide 35. PF 5 phosphorus pentafluoride 36. Mn(ClO) 2 manganese (II) hypochlorite 37. BrCl 3 bromine trichloride 38. Cr(NO 3 ) 3 chromium (III) nitrate 39. CoCO 3 cobalt (II) carbonate 40. NCl 3 nitrogen trichloride 41. BaSO 3 barium sulfite 42. CuClO copper (I) hypochlorite 43. P 4 O 10 tetraphosphorus decoxide 44. Ni(C 2 H 3 O 2 ) 2 nickel (II) acetate 33

34 CHM130 Practice (Single Replacement Reaction) Name: i) Write balanced formula equation for each of the following reactions. Explain why this reaction occurs. i Write word equation. 1. i) Al + HCl i 2. i) AgNO 3 + Mg i 3. i) H 3 PO 4 + Li i 4. i) Mn + PbBr 2 i 5. i) Fe 2 (CO 3 ) 3 + Ca i 34

35 CHM130 Practice (Single Replacement reaction) Name: Write balanced formula equations for the following single replacement reactions. If no reaction occurs, write NR. i) Na + AgNO 3 H 2 SO 4 + Mg i Fe + NiCl 2 iv) K 2 CO 3 + Ba v) K + H 2 O vi) Al + Fe(NO 3 ) 2 v NaCl + Br 2 vi LiBr + Cl 2 CHM130 35

36 Practice (Double Replacement Reaction) Name: Write balanced formula equations for the following double replacement reactions. If no reaction occurs, write NR. a) NaOH + H 2 SO 4 b) AgNO 3 + HCl c) K 2 CO 3 + ZnBr 2 d) NH 4 I + LiOH e) HC 2 H 3 O 2 + Na 2 SO 3 f) KCl + Mg(NO 3 ) 2 36

37 CHM130 Practice (Reactions) Name: Write balanced formula equations for the following and classify each of these reactions as combination, decomposition, single replacement, or double replacement reaction. If no reaction occurs, write NR. a) sodium + iron(ii) nitrate b) copper(ii) chloride + potassium hydroxide c) ammonium chloride + sodium iodide d) Mg(C 2 H 3 O 2 ) 2 + H 2 CO 3 e) K + HgCl 2 f) H 2 + O 2 H 2 O g) H 2 SO 4 + Na 2 CO 3 h) KClO 3 KCl + O 2 i) MgO + H 2 O Mg(OH) 2 j) silver nitrate + sodium chloride k) iron(ii) bromide + sodium CHM130 37

38 Practice (Reactions) Name: Complete the following i) word equations and write balanced formula equations. i Classify each of these reactions as combination, decomposition, single replacement, or double replacement reaction. If no reaction occurs, write NR. a) i) lead(ii) nitrate + potassium chloride i b) i) silver hydroxide silver oxide + water i c) i) barium + chromium(iii) chloride i d) i) iron(iii) nitrate + potassium hydroxide i e) i) sodium carbonate + sulfuric acid i f) i) sodium sulfite + sulfuric acid i) i 38

39 h) i) phosphoric acid + potassium hydroxide i i) i) hydrochloric acid + potassium hydroxide i j) i) copper + silver nitrate i k) i) ammonium acetate + sodium hydroxide i l) i) hydrosulfuric acid + aluminum i m) i) iron(iii) bromide + phosphoric acid i n) i) cadmium(ii) acetate + barium bromide i 39

40 CHM130 Practice (Chemical quantities) Name: 1. Find the mass (in grams) of 2.45 moles of gold atoms. 2. How many copper atoms are in 2.35 x 10 4 grams of copper metal? 3. What is the mass (in grams) of 6.44 x molecules of P 4 O 10? 4. a) Give the mass of each of the following. Make sure to include unit. 1 mole of N atoms 1 mole of H atoms 1 mole of S atoms 1 mole of O atoms b) Determine the molar mass of ammonium sulfate. g/mol c) Calculate the mass percent composition of ammonium sulfate. % N: % H: % S: % O: 40

41 5. Calculate moles of hydrogen atoms that are contained in 34.5 g of ammonia (NH 3 ). 8. How many CO 2 molecules are contained in 1.25 x 10 3 g of CO 2? moles of H atoms CO 2 molecules 9. Calculate the mass (in grams) of nitrogen atoms in 4.50 moles of Mg(NO 3 ) 2. g of N atoms 10. Calculate the mass (in grams) of nitrogen atoms in 45.8 grams of dinitrogen monoxide (N 2 O). g N 41

42 CHM130 Practice (Determination of chemical formulas) Name: 1. Acetylene used in gas welding contains g C and 7.75 g H and has a molar mass of g/mole. a) Obtain the Empirical formula for acetylene. b) Find the molecular formula for acetylene. Empirical formula Molecular formula 2. Percent composition of a compound containing carbon, hydrogen, and oxygen is available as follows % C, 9.15% H The molar mass of the compound is g/mole. What are the empirical and molecular formulas for this compound? Empirical formula Molecular formula 42

43 3. Th elemental mass percents of a compound are 40.00% carbon, 6.72% hydrogen, and 53.28% oxygen. The molar mass of the compound is g. What are the empirical and molecular formulas for this compound? Empirical formula Molecular formula 4. Percent composition of a compound by mass is % carbon, 4.07 % hydrogen, 71.65% chlorine. i) Determine the empirical formula. Empirical formula Molar mass of the compound is g/mole. What is the molecular formula of this compound? Molecular formula 43

44 CHM130 Practice (Stoichiometry) 1. Aluminum oxide was prepared by reacting 2.50 g of aluminum and 2.50 g of oxygen. 4Al + 3O 2 2Al 2 O 3 a) Calculate the theoretical yield of aluminum oxide in this reaction and identify the limiting reactant. b) Determine the percent yield if 4.25 g of aluminum oxide was obtained grams of NaCl and 41.0 grams of AgNO 3 were allowed to react according to the following equation: NaCl + AgNO 3 AgCl + NaNO 3 a) What is the theoretical yield of NaNO 3? b) Identify the limiting reactant. 44

45 3. For the following reaction; NH 3 + F 2 N 2 F 4 + HF i) Balance the equation: How many moles of NH 3 are needed to produce 20.0 g of N 2 F 4? i How many grams of F 2 are required to react with 12.0 g of N 2? 4. For the combustion of octane; C 8 H 18 + O 2 i) Write a balanced formula equation. Suppose g of octane is combined with 60.0 g of oxygen. What is the theoretical yield of H 2 O? i Which one is a limiting reactant? 5. For the following reaction, CH 4 (methane) + 2O 2 2H 2 O + CO 2 i) How many grams of oxygen will be required to react with 4.55 moles of methane? How many grams of H 2 O will be produced if 33.2 grams of methane is reacted? 6. A reaction mixture contains 10.0 grams of Na and 2.35 grams of hydrogen for the following reaction: 2Na + H 2 2NaH 45

46 i) What is the theoretical yield of sodium hydride for the reaction? Which one is the limiting reactant? i When the reaction was performed, 8.50 grams of NaH was recovered. What is the percent yield of the reaction? 46

47 CHM130 Practice (Solution) Name: 1. Identify each of the following as an electrolyte or a nonelectrolyte. a) solid KBr b) sugar(c 12 H 22 O 11 ) solution c) NaNO 3 (aq) d) KOH (aq) 2. A solution has a ph of 8.0. a) Is this solution an acidic solution or a basic solution? b) Which ion does this solution have more, H + or OH -? c) If this is not a buffer solution, what happens in ph of this solution when small amount of base is added to the solution? 3. Draw Lewis structures of the following molecules. a) NCl 3 b) H 2 S c) OF 2 d) CHCl 3 47