Slide 1 / 90. Slide 2 / 90. Slide 3 / 90 A B. percent yield stoichiometry A B. atoms and mass

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1 Stoichiometry HW Slide 1 / 90 Grade:«grade» Subject: ate:«date» 1 The calculation of quantities in chemical equations is called. Slide 2 / 90 accuracy and precision dimensional analysis percent composition percent yield stoichiometry 2 What is conserved in the reaction shown below? H 2 (g) + l 2 (g) 2Hl(g) Slide 3 / 90 only mass only mass and moles only mass, moles, and molecules only mass, moles, molecules and volume atoms and mass

2 3 What is conserved in the reaction shown below? N 2 (g) + 3F 2 (g) 2NF 3 (g) Slide 4 / 90 only atoms only mass only mass and atoms only moles only mass, atoms, moles, and molecules 4 In every chemical reaction, Slide 5 / 90 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 5 Which of the following statements is true about the total number of reactants and the total number of products in this reaction? 5 H 12 (l) + 8O 2 (g) 5O 2 (g) + 6H 2 O(g) Slide 6 / 90 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

3 6 Which of these is an INORRT interpretation of this balanced equation? 2S(s) + 3O 2 (g) 2SO 3 (g) Slide 7 / 90 2 atoms S + 3 molecules O 2 2 molecules SO 3 2 g S + 3 g O 2 2 g SO 3 2 mol S + 3 mol O 2 2 mol SO 3 2 L S + 3L O 2 2L SO 3 none of the above 7 In a chemical reaction the mass of the products Slide 8 / 90 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 8 In any chemical reaction the quantities that are preserved are Slide 9 / 90 the number of moles and the volumes the number of molecules and the volumes mass and number of atoms mass and moles mass only

4 9 Which of the following statements is true about the following reaction? Slide 10 / 90 3NaHO 3(aq) + 6H 8O 7(aq) 3O 2(g) + 3H 2O(s) +Na 3 6H 5O 7(aq) 22.4 L of O 2(g) are produced for every liter of 6H 8O 7(aq) reacted 1 mole of water is produced for every mole of carbon dioxide produced 6.02 x 1023 molecules of Na 3 6H 5O 7(aq) are produced for every mole of NaHO 3(aq) used 54 g of water is produced for every mole of NaHO 3(aq) produced 10 In the reaction 2O(g) + O 2 (g) 2O 2 (g), what is the ratio of moles of oxygen used to moles of O 2 produced? Slide 11 / 90 1:1 2:1 1:2 2:2 11 The combustion of propane ( 3 H 8 ) produces O 2 and H 2 O: 3 H 8 (g) + 5O 2 (g) 3O 2 (g) + 4H 2 O (l) The reaction of 2.5 mol of O 2 will produce mol of H 2 O. Slide 12 /

5 12 The combustion of propane ( 3 H 8 ) in the presence of excess oxygen yields O 2 and H 2 O: 3 H 8 (g) + 5O 2 (g) 3O 2 (g) + 4H 2 O When 2.5 mol of O 2 are consumed in their reaction, mol of O 2 are produced. Slide 13 / 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? Slide 14 / 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? Slide 15 /

6 15 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? Slide 16 / 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? Slide 17 / utomotive 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? Slide 18 /

7 18 How many moles of aluminum are needed to react completely with 3.2 mol of FeO? 2l(s) + 3FeO(s) 3Fe(s) + l 2 O 3 (s) Slide 19 / mol 2.1 mol 1.6 mol 6.4 mol 4.8 mol 19 alculate the number of moles of l 2 O 3 that are produced when 15 mol of Fe is produced in the following reaction. 2l(s) + 3FeO(s) 3Fe(s) + l 2 O 3 (s) Slide 20 / 90 5 mol 15 mol 45 mol 7.5 mol 30 mol 20 How many moles of glucose, 6 H 12 O 6, can be burned when 60.0 mol of oxygen is available? 6 H 12 O 6 (s) + 6O 2 (g) 6O 2 (g) + 6H 2 O(l) Slide 21 / mol 10 mol 60 mol 120 mol 301 mol

8 21 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? 2l(s) + 3H 2 SO 4 (aq) l 2 (SO 4 ) 3 (aq) + 3H 2 (g) Slide 22 / mol 10.0 mol 25.0 mol 37.5 mol 75 mol 22 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) Slide 23 / mol 1.8 mol 2.4 mol 3.2 mol 4.8 mol 23 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) Slide 24 / mol 1.00 mol 4.00 mol 16.0 mol 98.0 mol

9 24 alcium carbide (a 2 ) reacts with water to produce acetylene ( 2 H 2 ): a 2 (s) + 2H 2 O (g) a(oh 2 ) (s) + 2 H 2 (g) Production of 13 g of 2 H 2 requires consumption of g of H 2 O. Slide 25 / x x 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. Slide 26 / 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. Slide 27 /

10 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 43.9 g of ammonia produces g of NO 2. Slide 28 / Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N 2 (g) + 3H 2 (g) 2NH 3 (g) 7.1-g sample of N 2 requires g of H 2 for complete reaction. Slide 29 / Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbO 3 (s) PbO (s) O 2 (g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate? Slide 30 /

11 30 The combustion of propane ( 3 H 8 ) in the presence of excess oxygen yields O 2 and H 2 O: 3 H 8 (g) + 5O 2 (g) 3O 2 (g) + 4H 2 O When 7.3 g of 3 H 8 burns in the presence of excess O 2, g of O 2 is produced. Slide 31 / Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N 2 (g) + 3H 2 (g) 2NH 3 (g) 9.3-g sample of hydrogen requires g of N 2 for a complete reaction. Slide 32 / Water can be formed from the stoichiometric reaction of hydrogen with oxygen: 2H 2 (g) + O 2 (g) 2H 2 O (g) complete reaction of 5.0 g of O 2 with excess hydrogen produces g of H 2 O. Slide 33 / 90

12 33 The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide: S 2 (g) + 3 O 2 (g) O 2 (g) + 2SO 2 (g) The combustion of 15 g of S 2 in the presence of excess oxygen yields g of SO 2. Slide 34 / utomotive 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? Slide 35 / 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. Slide 36 /

13 36 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) Slide 37 / g 23.9 g 47.8 g 95.6 g 267 g 37 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 6 H 12 O 6 completely reacted with oxygen? Slide 38 / g 1.8 g 11 g 66 g 12,000 g 38 luminum 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? 2l(s) + 3H 2 SO 4 (aq) l 2 (SO 4 ) 3 (aq) + 3H 2 (g) Slide 39 / g 290 g 450 g 870 g 2600 g

14 39 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) + 4aO(s) 4Hg(l) + 3aS(s) + aso 4 (s) Slide 40 / g 7.56 g 10.1 g 13.4 g 36.0 g 40 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) Slide 41 / L 3.6 L 2.0 L 2.4 L 7.2 L 41 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) Slide 42 / g 2.00 g 2.88 g 32.0 g 46.0 g

15 42 How many grams of beryllium are needed to produce 36.0 g of hydrogen? (ssume an excess of water) e(s) + 2H 2 O(l) e(oh) 2 (aq) + H 2 (g) Slide 43 / g 36.0 g 162 g 324 g 648 g 43 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) Slide 44 / L 2.12 L 3.03 L 6.49 L 77.3 L 44 How many liters of hydrogen gas are needed to react with S 2 to produce 2.50 L of H 4, at STP? 4H 2 (g) + S 2 (l) H 4 (g) + 2H 2 S(g) Slide 45 / L L 5.00 L 7.50 L 10.0 L

16 45 How many liters of chlorine gas can be produced when 0.98 L of Hl react with excess O 2, at STP? 4Hl(g) + O 2 (g) 2l 2 (g) + 2H 2 O(g) Slide 46 / L 0.49 L 3.9 L 2.0 L 0.25 L 46 Which conversion factor do you use first to calculate the number of grams of O 2 produced by the reaction of 50.6 g of H 4 with O 2? The equation for the complete combustion of methane is: H 4 (g) + 2O 2 (g) O 2 (g) + 2H 2 O(l) Slide 47 / 90 (1 mol H 4 /16.0 g H 4 ) (2 mol O 2 /1 mol O 2 ) (16.0 g H 4 /1 mol O 4 ) (44.0 g O 2 /2 mol O 2 ) (1 mol O 2 /44 g O 2 ) 47 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) Slide 48 / L 20.0 L 7.5 L L L

17 48 Glucose, 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 O 2 are produced when 126 g of glucose completely reacts with oxygen? 6 H 12 O 6 (s) + 6O 2 (g) 6O 2 (g) + 6H 2 O(l) kcal Slide 49 / L 5.33 L 15.7 L 94.1 L 185 L 49 alcium oxide, or lime, is produced by the thermal decomposition of limestone in the reaction: ao 3 (s) ao(s) + O 2 (g). What mass of lime can be produced from 1.5 x 10 3 kg of limestone? Slide 50 / x 10 5 kg 8.4 x 10 2 kg 8.4 kg Not enough information given. 50 When two substances react to form products, the reactant which is used up is called the. Slide 51 / 90 determining reagent limiting reagent excess reagent catalytic reagent reactive reagent

18 51 Which of the following is NOT a true statement concerning limiting and excess reagents? Slide 52 / 90 The amount of product obtained is determined by the limiting reagent. 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. dding more of the limiting reagent to the reaction chamber will cause more product to be produced. 52 When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the. Slide 53 / 90 ctual Yield Percent Yield Theoretical Yield Minimum Yield Percent omposition 53 Which of the following is NOT a true statement about "yield"? Slide 54 / 90 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.

19 54 For a given chemical reaction, the theoretical yield is greater than the actual yield. Slide 55 / 90 sometimes always never 55 The reagent present in the smallest amount is the limiting reagent. Slide 56 / 90 always sometimes never 56 Which of the following is not a reason why actual yield is less than theoretical yield? Slide 57 / 90 impure reactants present competing side reactions loss of product during purification conservation of mass

20 57 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) Slide 58 / Silver nitrate and aluminum chloride react with each other by exchanging anions: 3gNO 3 (aq) + ll 3 (aq) l(no 3 ) 3 (aq) + 3gl(s) What mass in grams of gl is produced when 4.22 g of gno 3 react with 7.73 g of ll 3? Slide 59 / The quantity of product that is calculated to form when all of the limiting reagent reacts is called the actual yield. T/F Slide 60 / 90

21 60 Pentacarbonyliron Fe(O) 5 reacts with phosphorous trifluoride (PF 3 ) and hydrogen, releasing carbon monoxide: Fe(O) 5 + PF 3 + H 2 Fe(O) 2 (PF3) 2 (H) 2 + O (not balanced) The reaction of 5.0 mol of Fe(O) 5, 8.0 mol of PF 3 and 6.0 mol of H 2 will release mol of O. Slide 61 / 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) Slide 62 / 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) Slide 63 /

22 63 Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4l (s) + 3O 2 (g) 2l 2 O 3 (s) The maximum amount of l 2 O 3 that can be produced from 2.5 g of l and 2.5 g of O 2 is g. Slide 64 / 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. Slide 65 / 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. Slide 66 /

23 66 alcium oxide reacts with water in a combination reaction to produce calcium hydroxide: ao (s) + H 2 O (l) a(oh) 2 (s) 4.50-g sample of ao is reacted with 4.34 g of H 2 O. How many grams of water remain after completion of reaction? Slide 67 / 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 Slide 68 / 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 Slide 69 /

24 69 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) Slide 70 / g 6.7 g 147 g 653 g 1180 g 70 How many grams of chromium are needed to react with an excess of uso 4 to produce 27.0 g u? 2r(s) + 3uSO 4 (aq) r 2 (SO 4 ) 3 (aq) + 3u(s) Slide 71 / g 14.7 g 18.0 g 33.2 g 81.5 g 71 Identify the limiting reagent and the volume of product formed when 11 L S 2 reacts with 18 L O 2 to produce O 2 gas and SO 2 gas. S 2 (g) + 3O 2 (g) O 2 (g) + 2SO 2 (g) Slide 72 / 90 S 2 ; 5.5 L O 2 O 2 ; 6.0 L O 2 S 2 ; 11 L O 2 O 2 ; 27 L SO 2 O 2 ; 54 L O 2

25 72 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) Slide 73 / g 6.8 g 270 g 45 g 99 g 73 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 S 2. 4H 2 (g) + S 2 (g) H 4 (g) + 2H 2 S(g) Slide 74 / 90 3 L S 2 6 L S 2 9 L S 2 12 L H 2 24 L H 2 74 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 l reacts with 319 g of uso 4? 2l + 3uSO 4 l 2 (SO 4 ) 3 + 3u Slide 75 / g 127 g 162 g 381 g 957 g

26 75 Which statement is true if 12 mol O and 12 mol Fe 2 O 3 are allowed to react? 3O(g) + Fe 2 O 3 (s) 2Fe(s) + 3O 2 (g) Slide 76 / 90 The limiting reagent is O and 8.0 mol Fe will be formed. The limiting reagent is O and 3.0 mol O 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 O 2 will be formed. The limiting reagent is Fe and 18 mol O 2 will be formed. 76 Which of the following would be the limiting reagent in the reaction: 2H 2 (g) + O 2 (g) 2H 2 O(g) Slide 77 / molecules of H 2 50 molecules of O 2 Neither nor is limiting. 77 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)? Slide 78 / 90 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.

27 78 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? Slide 79 / 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? Slide 80 / 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. Slide 81 /

28 81 Propane ( 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? Slide 82 / Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4l (s) + 3O 2 (g) 2l 2 O 3 (s) In a particular experiment, the reaction of 2.5 g of l with 2.5 g of O 2 produced 3.5 g of l 2 O 3. The % yield of the reaction is. Slide 83 / alcium oxide reacts with water in a combination reaction to produce calcium hydroxide: ao(s) + H 2 O(l) a(oh) 2 (s) In a particular experiment, a 5.00-g sample of ao is reacted with excess water and 6.11 g of a(oh) 2 is recovered. What is the percent yield in this experiment? Slide 84 /

29 84 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. Slide 85 / 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) Slide 86 / 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) Slide 87 / 90 18% 44% 56% 67% 82%

30 87 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) + 2Hl(aq) Znl 2 (s) + H 2 (g) Slide 88 / g 95 g 180 g 280 g 380 g 88 In a particular reaction between copper metal and silver nitrate, 13 g u produced 40 g g. What is the percent yield of silver in this reaction? u + 2gNO 3 u(no 3 ) 2 + 2g Slide 89 / % 56.7% 77.3% 90.6% 176% Slide 90 / 90

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

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date» Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date» Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent