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1 Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date»

2 Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent composition percent yield stoichiometry

3 Slide 3 / 90 2 What is conserved in the reaction shown below? H 2 (g) + Cl 2 (g) 2HCl(g) A B C D E only mass only mass and moles only mass, moles, and molecules only mass, moles, molecules and volume atoms and mass

4 Slide 4 / 90 3 What is conserved in the reaction shown below? N 2 (g) + 3F 2 (g) 2NF 3 (g) A B C D E only atoms only mass only mass and atoms only moles only mass, atoms, moles, and molecules

5 Slide 5 / 90 4 In every chemical reaction, A B C D E mass and molecules are conserved moles and liters are conserved mass and atoms are conserved moles and molecules are conserved mass and liters are conserved

6 Slide 6 / 90 5 Which of the following statements is true about the total number of reactants and the total number of products in this reaction? C 5 H 12 (l) + 8O 2 (g) 5CO 2 (g) + 6H 2 O(g) A B C D E 9 moles of reactants regroup to form 11 moles of product 9 grams of reactants regroup to form 11 grams of product 9 liters of reactants regroup to form 11 liters of product 9 atoms of reactants regroup to form 11 atoms of product 22.4 liters of reactants regroup to form 22.4 liters of product

7 Slide 7 / 90 6 Which of these is an INCORRECT interpretation of this balanced equation? 2S(s) + 3O 2 (g) 2SO 3 (g) A 2 atoms S + 3 molecules O 2 2 molecules SO 3 B 2 g S + 3 g O 2 2 g SO 3 C 2 mol S + 3 mol O 2 2 mol SO 3 D 2 L S + 3L O 2 2L SO 3 E none of the above

8 Slide 8 / 90 7 In a chemical reaction the mass of the products A B C D E is less than the mass of the reactants is greater than the mass of the reactants is equal to the mass of the reactants has no relationship to the mass of the reactants depends on the reaction equation

9 Slide 9 / 90 8 In any chemical reaction the quantities that are preserved are A B C D E the number of moles and the volumes the number of molecules and the volumes mass and number of atoms mass and moles mass only

10 Slide 10 / 90 9 Which of the following statements is true about the following reaction? 3NaHCO 3 (aq) + C 6 H 8 O 7 (aq) 3CO 2 (g) + 3H 2 O(s) +Na 3 C 6 H 5 O 7 (aq) A B C D 22.4 L of CO 2 (g) are produced for every liter of C 6 H 8 O 7 (aq) reacted 1 mole of water is produced for every mole of carbon dioxide produced 6.02 x 1023 molecules of Na 3 C 6 H 5 O 7 (aq) are produced for every mole of NaHCO 3 (aq) used 54 g of water is produced for every mole of NaHCO 3 (aq) produced

11 Slide 11 / In the reaction 2CO(g) + O 2 (g) 2CO 2 (g), what is the ratio of moles of oxygen used to moles of CO 2 produced? A 1:1 B 2:1 C 1:2 D 2:2

12 Slide 12 / The combustion of propane (C 3 H 8 ) produces CO 2 and H 2 O: C 3 H 8 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O (l) The reaction of 2.5 mol of O 2 will produce mol of H 2 O. A 4.0 B 3.0 C 2.5 D 2.0 E 1.0

13 Slide 13 / The combustion of propane (C 3 H 8 ) in the presence of excess oxygen yields CO 2 and H 2 O: C 3 H 8 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O When 2.5 mol of O 2 are consumed in their reaction, mol of CO 2 are produced. A 1.5 B 3.0 C 5.0 D 6.0 E 2.5

14 Slide 14 / Lithium and nitrogen react to produce lithium nitride: 6Li (s) + N 2 (g) 2Li 3 N (s) How many moles of N 2 are needed to react with mol of lithium? A 3.00 B C D 1.50 E

15 Slide 15 / Lithium and nitrogen react to produce lithium nitride: 6Li (s) + N 2 (g) 2Li 3 N (s) How many moles of lithium nitride are produced when 0.30 mol of lithium react in this fashion? A B C D 1.35 E 0.225

16 Slide 16 / Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N 2 (g) 2Li 3 N (s) How many moles of lithium are needed to produce 0.50 mol of Li 3 N when the reaction is carried out in the presence of excess nitrogen? A 0.30 B 1.50 C 0.20 D 0.40 E 3.6

17 Slide 17 / Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O 2 (g) 2MgO (s) How many moles of O 2 are consumed when mol of magnesium burns? A B 2.60 C D 1.54 E 0.44

18 Slide 18 / Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN 3 (s) 2Na (s) + 3N 2 (g) How many moles of N 2 are produced by the decomposition of 5.25 mol of sodium azide? A 5.25 B 8.64 C 7.88 D E 1.44

19 Slide 19 / How many moles of aluminum are needed to react completely with 3.2 mol of FeO? 2Al(s) + 3FeO(s) 3Fe(s) + Al 2 O 3 (s) A B C D E 3.2 mol 2.1 mol 1.6 mol 6.4 mol 4.8 mol

20 Slide 20 / Calculate the number of moles of Al 2 O 3 that are produced when 15 mol of Fe is produced in the following reaction. 2Al(s) + 3FeO(s) 3Fe(s) + Al 2 O 3 (s) A B C D E 5 mol 15 mol 45 mol 7.5 mol 30 mol

21 Slide 21 / How many moles of glucose, C 6 H 12 O 6, can be burned when 60.0 mol of oxygen is available? C 6 H 12 O 6 (s) + 6O 2 (g) 6CO 2 (g) + 6H 2 O(l) A B C D E mol 10 mol 60 mol 120 mol 301 mol

22 Slide 22 / Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 25.0 mol of aluminum? 2Al(s) + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) A B C D E mol 10.0 mol 25.0 mol 37.5 mol 75 mol

23 Slide 23 / When iron rusts in air, iron(iii) oxide is produced. How many moles of oxygen react with 2.4 mol of iron? 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) A B C D E 1.2 mol 1.8 mol 2.4 mol 3.2 mol 4.8 mol

24 Slide 24 / How many moles of H 3 PO 4 are produced when 71.0 g P 4 O 10 reacts completely to form H 3 PO 4? P 4 O 10 (s) + 6H 2 O(l) 4H 3 PO 4 (aq) A B C D E mol 1.00 mol 4.00 mol 16.0 mol 98.0 mol

25 Slide 25 / Calcium carbide (CaC 2 ) reacts with water to produce acetylene (C 2 H 2 ): CaC 2 (s) + 2H 2 O (g) Ca(OH 2 ) (s) + C 2 H 2 (g) Production of 13 g of C 2 H 2 requires consumption of g of H 2 O. A 4.5 B 9.0 C 18 D 4.8x10 2 E 4.8x10-2

26 Slide 26 / Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3Mg + N 2 Mg 3 N 2 In a particular experiment, a 10 g sample of N 2 reacts completely. The mass of Mg consumed is g. A 8.04 B 26.0 C 16.1 D 0.92 E 13.9

27 Slide 27 / The combustion of ammonia in the presence of excess oxygen yields NO 2 and H 2 O: 4NH 3 (g) + 7O 2 (g) 4NO 2 (g) + 6H 2 O (g) The combustion of 28.8 g of ammonia consumes g of oxygen. A 94.7 B 54.1 C 108 D 15.3 E 28.8

28 Slide 28 / The combustion of ammonia in the presence of excess oxygen yields NO 2 and H 2 O: 4NH 3 (g) + 7O 2 (g) 4NO 2 (g) + 6H 2 O (g) The combustion of 43.9 g of ammonia produces g of NO 2. A 2.58 B 178 C 119 D E 43.9

29 Slide 29 / Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N 2 (g) + 3H 2 (g) 2NH 3 (g) A 7.1-g sample of N 2 requires g of H 2 for complete reaction. A 0.51 B 0.76 C 1.2 D 1.5 E 17.2

30 Slide 30 / Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO 3 (s) PbO (s) CO 2 (g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate? A 0.41 B 2.50 C D 2.09 E 2.61

31 Slide 31 / The combustion of propane (C 3 H 8 ) in the presence of excess oxygen yields CO 2 and H 2 O: C 3 H 8 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O When 7.3 g of C 3 H 8 burns in the presence of excess O 2, g of CO 2 is produced.

32 Slide 32 / Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N 2 (g) + 3H 2 (g) 2NH 3 (g) A 9.3-g sample of hydrogen requires g of N 2 for a complete reaction.

33 Slide 33 / Water can be formed from the stoichiometric reaction of hydrogen with oxygen: 2H 2 (g) + O 2 (g) 2H 2 O (g) A complete reaction of 5.0 g of O 2 with excess hydrogen produces g of H 2 O.

34 Slide 34 / The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide: CS 2 (g) + 3 O 2 (g) CO 2 (g) + 2SO 2 (g) The combustion of 15 g of CS 2 in the presence of excess oxygen yields g of SO 2.

35 Slide 35 / Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN 3 (s) 2Na (s) + 3N 2 (g) How many grams of sodium azide are required to produce 33.0 g of nitrogen? A 1.77 B C 76.6 D 51.1 E 114.9

36 Slide 36 / Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O 2 (g) 2MgO (s) When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is g. A 4.00 B 6.63 C D 3.32 E 13.3

37 Slide 37 / Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe 2 O 3 are formed when 16.7 g of Fe reacts completely with oxygen? 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) A B C D E 12.0 g 23.9 g 47.8 g 95.6 g 267 g

38 Slide 38 / When glucose is consumed it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of C 6 H 12 O 6 completely reacted with oxygen? A B C D E 1.5 g 1.8 g 11 g 66 g 12,000 g

39 Slide 39 / Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many grams of aluminum sulfate would be formed if 250 g H 2 SO 4 completely reacted with aluminum? 2Al(s) + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) A B C D E 0.85 g 290 g 450 g 870 g 2600 g

40 Slide 40 / Mercury can be obtained by reacting mercury(ii) sulfide with calcium oxide. How many grams of calcium oxide are needed to produce 36.0 g of Hg? 4HgS(s) + 4CaO(s) 4Hg(l) + 3CaS(s) + CaSO 4 (s) A B C D E 1.80 g 7.56 g 10.1 g 13.4 g 36.0 g

41 Slide 41 / How many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water? 2H 2 (g) + O 2 (g) 2H 2 O(g) A B C D E 1.8 L 3.6 L 2.0 L 2.4 L 7.2 L

42 Slide 42 / The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO 2 is formed? 2Pb(NO 3 ) 2 (s) 2PbO(s) + 4NO 2 (g) + O 2 (g) A B C D E 1.00 g 2.00 g 2.88 g 32.0 g 46.0 g

43 Slide 43 / How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water) Be(s) + 2H 2 O(l) Be(OH) 2 (aq) + H 2 (g) A B C D E 4.00 g 36.0 g 162 g 324 g 648 g

44 Slide 44 / How many liters of NH 3, at STP, will react with 5.3g O 2 to form NO 2 and water? 4NH 3 (g) + 7O 2 (g) 4NO 2 + 6H 2 O(g) A B C D E 23 L 2.12 L 3.03 L 6.49 L 77.3 L

45 Slide 45 / How many liters of hydrogen gas are needed to react with CS 2 to produce 2.50 L of CH 4, at STP? 4H 2 (g) + CS 2 (l) CH 4 (g) + 2H 2 S(g) A B C D E 2.50 L L 5.00 L 7.50 L 10.0 L

46 Slide 46 / How many liters of chlorine gas can be produced when 0.98 L of HCl react with excess O 2, at STP? 4HCl(g) + O 2 (g) 2Cl 2 (g) + 2H 2 O(g) A B C D E 0.98 L 0.49 L 3.9 L 2.0 L 0.25 L

47 Slide 47 / Which conversion factor do you use first to calculate the number of grams of CO 2 produced by the reaction of 50.6 g of CH 4 with O 2? The equation for the complete combustion of methane is: CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) A (1 mol CH 4 /16.0 g CH 4 ) B (2 mol O 2 /1 mol CO 2 ) C (16.0 g CH 4 /1 mol CO 4 ) D (44.0 g CO 2 /2 mol CO 2 ) E (1 mol CO 2 /44 g CO 2 )

48 Slide 48 / How many liters of NH 3 are needed to react completely with 30.0 L of NO (at STP)? 4NH 3 (g) + 6NO(g) 5N 2 (g) + 6H 2 O(g) A B C D E 5.0 L 20.0 L 7.5 L L L

49 Slide 49 / Glucose, C 6 H 12 O 6, is a good source of food energy. When it reacts with oxygen, carbon dioxide, and water are formed. How many liters of CO 2 are produced when 126 g of glucose completely reacts with oxygen? C 6 H 12 O 6 (s) + 6O 2 (g) 6CO 2 (g) + 6H 2 O(l) kcal A B C D E 4.21 L 5.33 L 15.7 L 94.1 L 185 L

50 Slide 50 / Calcium oxide, or lime, is produced by the thermal decomposition of limestone in the reaction: CaCO 3 (s) CaO(s) + CO 2 (g). What mass of lime can be produced from 1.5 x 10 3 kg of limestone? A B C D 8.4 x 10 5 kg 8.4 x 10 2 kg 8.4 kg Not enough information given.

51 Slide 51 / When two substances react to form products, the reactant which is used up is called the. A B C D E determining reagent limiting reagent excess reagent catalytic reagent reactive reagent

52 Slide 52 / Which of the following is NOT a true statement concerning limiting and excess reagents? A B C D E The amount of product obtained is determined by the limiting reagent. A balanced equation is necessary to determine which reactant is the limiting reagent. Some of the excess reagent is left over after the reaction is complete. The reactant that has the smallest given mass is the limiting reagent. Adding more of the limiting reagent to the reaction chamber will cause more product to be produced.

53 Slide 53 / When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the. A B C D E Actual Yield Percent Yield Theoretical Yield Minimum Yield Percent Composition

54 Slide 54 / Which of the following is NOT a true statement about "yield"? A B C D E The value of the actual yield must be given in order for the percent yield to be calculated. The actual yield is often less than the theoretical yield. The percent yield is the ratio of the actual yield to the theoretical yield. The actual yield may be different from the theoretical yield because reactions do not always go to completion. The actual yield may be different from the theoretical yield because insufficient limiting reagent was used.

55 Slide 55 / For a given chemical reaction, the theoretical yield is greater than the actual yield. A B C sometimes always never

56 Slide 56 / The reagent present in the smallest amount is the limiting reagent. A B C always sometimes never

57 Slide 57 / Which of the following is not a reason why actual yield is less than theoretical yield? A B C D impure reactants present competing side reactions loss of product during purification conservation of mass

58 Slide 58 / What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2H 2 O (l) Mg(OH) 2 (s) + H 2 (g) A B C D E 0.204

59 Slide 59 / Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO 3 (aq) + AlCl 3 (aq) Al(NO 3 ) 3 (aq) + 3AgCl(s) What mass in grams of AgCl is produced when 4.22 g of AgNO 3 react with 7.73 g of AlCl 3? A 17.6 B 4.22 C 24.9 D 3.56 E 11.9

60 Slide 60 / The quantity of product that is calculated to form when all of the limiting reagent reacts is called the actual yield. T/F

61 Slide 61 / Pentacarbonyliron Fe(CO) 5 reacts with phosphorous trifluoride (PF 3 ) and hydrogen, releasing carbon monoxide: Fe(CO) 5 + PF 3 + H 2 Fe(CO) 2 (PF3) 2 (H) 2 + CO (not balanced) The reaction of 5.0 mol of Fe(CO) 5, 8.0 mol of PF 3 and 6.0 mol of H 2 will release mol of CO. A 15 B 5.0 C 24 D 6.0 E 12

62 Slide 62 / What is the maximum mass in grams of NH 3 that can be produced by the reaction of 1.0 g of N 2 with 3.0 g of H 2 via the equation below? N 2 (g) + H 2 (g) NH 3 (g) (not balanced) A 2.0 B 1.2 C 0.61 D 17 E 4.0

63 Slide 63 / What is the maximum amount in grams of SO 3 that can be produced by the reaction of 1.0 g of S with 1.0 g of O 2 via the equation below? S (s) + O 2 (g) SO 3 (g) (not balanced) A 0.27 B 1.7 C 2.5 D 3.8 E 2.0

64 Slide 64 / Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O 2 (g) 2Al 2 O 3 (s) The maximum amount of Al 2 O 3 that can be produced from 2.5 g of Al and 2.5 g of O 2 is g. A 9.4 B 7.4 C 4.7 D 5.3 E 5.0

65 Slide 65 / Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F 2 (g) SF 6 (g) The maximum amount of SF6 that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is g. A 12 B 3.2 C 5.8 D 16 E 8.0

66 Slide 66 / Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N 2 (g) 2Li 3 N (s) In a particular experiment, 3.50 g samples of each reagent are reacted. The theoretical yield of lithium nitride is g. A 3.52 B 2.93 C 17.6 D 5.85 E 8.7

67 Slide 67 / Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H 2 O (l) Ca(OH) 2 (s) A 4.50-g sample of CaO is reacted with 4.34 g of H 2 O. How many grams of water remain after completion of reaction? A 0.00 B C 2.90 D 1.04 E 0.161

68 Slide 68 / If 294 grams of FeS 2 is allowed to react with 176 grams of O 2 according to the following equation, how many grams of Fe 2 O 3 are produced? FeS 2 + O 2 Fe 2 O 3 + SO 2

69 Slide 69 / How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride with 7.73 g of water? Mg 3 N 2 + 3H 2 O 2NH 3 + 3MgO A B C D E 4.57

70 Slide 70 / How many grams of H 3 PO 4 are produced when 10.0 moles of water react with an excess of P 4 O 10? P 4 O 10 (s) + 6H 2 O(l) 4H 3 PO 4 (aq) A B C D E 1.22 g 6.7 g 147 g 653 g 1180 g

71 Slide 71 / How many grams of chromium are needed to react with an excess of CuSO 4 to produce 27.0 g Cu? 2Cr(s) + 3CuSO 4 (aq) Cr 2 (SO 4 ) 3 (aq) + 3Cu(s) A B C D E 48.0 g 14.7 g 18.0 g 33.2 g 81.5 g

72 Slide 72 / Identify the limiting reagent and the volume of product formed when 11 L CS 2 reacts with 18 L O 2 to produce CO 2 gas and SO 2 gas. CS 2 (g) + 3O 2 (g) CO 2 (g) + 2SO 2 (g) A CS 2 ; 5.5 L CO 2 B O 2 ; 6.0 L CO 2 C CS 2 ; 11 L CO 2 D O 2 ; 27 L SO 2 E O 2 ; 54 L CO 2

73 Slide 73 / What is the maximum number of grams of PH 3 that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PH 3? P 4 (g) + 6H 2 (g) 4PH 3 (g) A B C D E 0.43 g 6.8 g 270 g 45 g 99 g

74 Slide 74 / Methane and hydrogen sulfide form when hydrogen reacts with carbon disulfide. Identify the excess reagent and calculate how much remains after 36 L of H 2 reacts with 12 L of CS 2. 4H 2 (g) + CS 2 (g) CH 4 (g) + 2H 2 S(g) A 3 L CS 2 B 6 L CS 2 C 9 L CS 2 D 12 L H 2 E 24 L H 2

75 Slide 75 / Metallic copper is formed when aluminum reacts with copper(ii) sulfate. How many grams of metallic copper can be obtained when 54.0 g of Al reacts with 319 g of CuSO 4? 2Al + 3CuSO 4 Al 2 (SO 4 ) 3 + 3Cu A B C D E 21.2 g 127 g 162 g 381 g 957 g

76 Slide 76 / Which statement is true if 12 mol CO and 12 mol Fe 2 O 3 are allowed to react? 3CO(g) + Fe 2 O 3 (s) 2Fe(s) + 3CO 2 (g) A B C D E The limiting reagent is CO and 8.0 mol Fe will be formed. The limiting reagent is CO and 3.0 mol CO 2 will be formed. The limiting reagent is Fe 2 O 3 and 24 mol Fe will be formed. The limiting reagent is Fe 2 O 3 and 36 mol CO 2 will be formed. The limiting reagent is Fe and 18 mol CO 2 will be formed.

77 Slide 77 / Which of the following would be the limiting reagent in the reaction: 2H 2 (g) + O 2 (g) 2H 2 O(g) A 50 molecules of H 2 B 50 molecules of O 2 C Neither A nor B is limiting.

78 Slide 78 / When 0.2 mol of calcium reacts with 880 g water, 2.24 L of hydrogen gas form (at STP). How would the amount of hydrogen produced change is the volume of water was decreased to 440 ml (440g)? A B C D Only one half of the volume of hydrogen would be produced. The volume of hydrogen produced would be the same. The volume of hydrogen produced would double. No hydrogen would be produced.

79 Slide 79 / GeF 3 H is formed from GeH 4 and GeF 4 in the combination reaction: GeH 4 + 3GeF 4 4GeF 3 H If the reaction yield is 92.6%, how many moles of GeF 4 are needed to produce 8.00 mol of GeF 3 H? A 3.24 B 5.56 C 6.48 D 2.78 E 2.16

80 Slide 80 / A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg 3 N 2 + 3H 2 O 2NH 3 + 3MgO The actual yield of MgO is 3.60 g. What is the percent yield in the reaction? A 94.5 B 78.7 C 46.6 D 49.4 E 99.9

81 Slide 81 / Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F 2 (g) SF 6 (g) In a particular experiment, the percent yield is 79.0%. This means that in this experiment, a g sample of fluorine yields g of SF 6. A 30.3 B 10.1 C 7.99 D 24.0 E 0.110

82 Slide 82 / Propane (C 3 H 8 ) reacts with oxygen in the air to produce carbon dioxide and water. In a particular experiment, 38.0 grams of carbon dioxide are produced from the reaction of grams of propane with excess oxygen. What is the % yield in this reaction? A 38.0 B 57.6 C 66.0 D 86.4 E 94.5

83 Slide 83 / Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O 2 (g) 2Al 2 O 3 (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O 2 produced 3.5 g of Al 2 O 3. The % yield of the reaction is. A 74 B 37 C 47 D 66 E 26

84 Slide 84 / Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H 2 O(l) Ca(OH) 2 (s) In a particular experiment, a 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH) 2 is recovered. What is the percent yield in this experiment? A 122 B 1.22 C 7.19 D 92.5 E 81.9

85 Slide 85 / Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s) + 3O 2 (g) 2SO 3 (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O 2 produced 0.80 g of SO 3. The % yield in this experiment is. A 30 B 29 C 21 D 88 E 48

86 Slide 86 / Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO 3 are produced by the reaction of 5.0 grams of O 2 with 6.0 grams of S. What is the % yield of SO 3 in this experiment? S(s) + O 2 (g) SO 3 (g) (not balanced) A 32 B 63 C 75 D 95 E 99

87 Slide 87 / Lead nitrate can be decomposed by heating. What is the percent yield of the decomposition reaction if 9.9 g Pb(NO 3 ) 2 is heated to give 5.5 g of PbO? 2Pb(NO 3 ) 2 (s) 2PbO(s) + 4NO 2 (g) + O 2 (g) A 18% B 44% C 56% D 67% E 82%

88 Slide 88 / Hydrogen gas is produced when zinc reacts with hydrochloric acid. If the actual yield of this reaction is 85%, how many grams of zinc are needed to produce 112 L of H 2 at STP? Zn(s) + 2HCl(aq) ZnCl 2 (s) + H 2 (g) A B C D E 2.2 g 95 g 180 g 280 g 380 g

89 Slide 89 / In a particular reaction between copper metal and silver nitrate, 13 g Cu produced 40 g Ag. What is the percent yield of silver in this reaction? Cu + 2AgNO 3 Cu(NO 3 ) 2 + 2Ag A 44.1% B 56.7% C 77.3% D 90.6% E 176%

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