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Ch12.1 - Stoichiometry N 2(g) + H 2(g) NH 3(g). Ch12.1 - Stoichiometry 1N 2(g) + 3H 2(g) 2NH 3(g) 1 mole reacts with 3 moles to produce 2 moles Masses:

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Presentation on theme: "Ch12.1 - Stoichiometry N 2(g) + H 2(g) NH 3(g). Ch12.1 - Stoichiometry 1N 2(g) + 3H 2(g) 2NH 3(g) 1 mole reacts with 3 moles to produce 2 moles Masses:"— Presentation transcript:

1 Ch Stoichiometry N 2(g) + H 2(g) NH 3(g)

2 Ch Stoichiometry 1N 2(g) + 3H 2(g) 2NH 3(g) 1 mole reacts with 3 moles to produce 2 moles Masses: = 28.0 g/mol = 2.0 g/mol = = g/mol How many moles of NH 3 produced? - 2 mol of N 2 react? - 1½ mol of H 2 react? - 28 g of N 2 react?

3 Ex1) Calculate the # of moles of nitrogen required to make 7.24 moles of ammonia. N H 2 2 NH 3 HW#1) Given 4 Al + 3 O 2 2 Al 2 O 3 a)How many moles of Al are needed to form 3.7 mol of Al 2 O 3 ? b) How many moles of O 2 are required to react completely with 14.8 moles of Al?

4 Ex1) Calculate the # of moles of nitrogen required to make 7.24 moles of ammonia. N H 2 2 NH 3 ? moles 7.24 moles 7.24 moles NH 3 1 moles N 2 2moles NH 3 = 3.62 moles N 2 HW#1) Given 4 Al + 3 O 2 2 Al 2 O 3 ? Mol 3.7 mol a)How many moles of Al are needed to form 3.7 mol of Al 2 O 3 ? 3.7 mol Al 2 O 3 4 mol Al 2 mol Al 2 O 3 = 7.4 mol Al b) How many moles of O 2 are required to react completely with 14.8 moles of Al? 14.8 mol Al3 mol O 2 4 mol Al= 11.1 mol O 2

5 Mass – Mass Calcs Ex2) Calculate the # of grams of NH 3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. N 2(g) + 3 H 2(g) 2 NH 3(g) Ex3) How many grams of nitrogen are needed to produce the 30.6g of NH 3 needed for the reaction? N 2(g) + 3 H 2(g) 2 NH 3(g)

6 Mass – Mass Calcs Ex2) Calculate the # of grams of NH 3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. N 2(g) + 3 H 2(g) 2 NH 3(g) 5.40 H 2 1 mol H 2 2 mol NH g NH g H 2 3 mol H 2 1 mol NH 3 = 30.6g NH 3 Ex3) How many grams of nitrogen are needed to produce the 30.6g of NH 3 needed for the reaction? N 2(g) + 3 H 2(g) 2 NH 3(g) 30.6g NH 3 1 mol NH 3 1 mol N g N g NH 3 2 mol NH 3 1 mol N 2 = 25.2g N 2

7 HW#2) CaC 2(s) + H 2 O C 2 H 2(g) + Ca(OH) 2(aq) a. How many moles of CaC 2 are needed to react completely with 49.0g of H 2 O? b. How many grams of Ca(OH) 2 are produced by 5.00g of CaC 2 ? c. How many grams of Ca(OH) 2 are produced when 0.89 mol of C 2 H 2 are produced?

8 HW#2) 1CaC 2(s) + 2H 2 O 1C 2 H 2(g) + 1Ca(OH) 2(aq) a. How many moles of CaC 2 are needed to react completely with 49.0g of H 2 O? 49.0g H 2 O 1 mol H 2 O 1 mol CaC g H 2 O 2 mol H 2 O= 1.36 moles CaC 2 b. How many grams of Ca(OH) 2 are produced by 5.00g of CaC 2 ? c. How many grams of Ca(OH) 2 are produced when 0.89 mol of C 2 H 2 are produced?

9 HW#2) 1CaC 2(s) + 2H 2 O 1C 2 H 2(g) + 1Ca(OH) 2(aq) a. How many moles of CaC 2 are needed to react completely with 49.0g of H 2 O? 49.0g H 2 O 1 mol H 2 O 1 mol CaC g H 2 O 2 mol H 2 O= 1.36 moles CaC 2 b. How many grams of Ca(OH) 2 are produced by 5.00g of CaC 2 ? 5.00g CaC 2 1 mol CaC 2 1 mol C 2 H g C 2 H g CaC 2 1 mol CaC 2 1 mol C 2 H 2 = 2.49g C 2 H 2 c. How many grams of Ca(OH) 2 are produced when 0.89 mol of C 2 H 2 are produced? CH 12 HW#1 1-3

10 HW#2) 1CaC 2(s) + 2H 2 O 1C 2 H 2(g) + 1Ca(OH) 2(aq) a. How many moles of CaC 2 are needed to react completely with 49.0g of H 2 O? 49.0g H 2 O 1 mol H 2 O 1 mol CaC g H 2 O 2 mol H 2 O= 1.36 moles CaC 2 b. How many grams of Ca(OH) 2 are produced by 5.00g of CaC 2 ? 5.00g CaC 2 1 mol CaC 2 1 mol C 2 H g C 2 H g CaC 2 1 mol CaC 2 1 mol C 2 H 2 = 2.49g C 2 H 2 c. How many grams of Ca(OH) 2 are produced when 0.89 mol of C 2 H 2 are produced?.89 mol C 2 H 2 1 mol Ca(OH) g Ca(OH) 2 1 mol C 2 H 2 1 mol Ca(OH) 2 = 66.0g Ca(OH) 2 CH 12 HW#1 1-3

11 Ch12 HW# ) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O a) How many grams of CO 2 & H 2 O are produced when 52.0g C 2 H 2 burn? CO 2 : H 2 O: b) How many grams O 2 to burn 52.0g C 2 H 2 ? c) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O

12 Ch12 HW# ) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O a) How many grams of CO 2 & H 2 O are produced when 52.0g C 2 H 2 burn? CO 2 : 52.0g C 2 H 2 1 mol C 2 H 2 4 mol CO g CO g C 2 H 2 2 mol C 2 H 2 1 mol CO 2 = 176 g CO 2 H 2 O: b) How many grams O 2 to burn 52.0g C 2 H 2 ? c) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O

13 Ch12 HW# ) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O a) How many grams of CO 2 & H 2 O are produced when 52.0g C 2 H 2 burn? CO 2 : 52.0g C 2 H 2 1 mol C 2 H 2 4 mol CO g CO g C 2 H 2 2 mol C 2 H 2 1 mol CO 2 = 176 g CO 2 H 2 O: 52.0g C 2 H 2 1 mol C 2 H 2 2 mol H 2 O 18.0g H 2 O 26.0 g C 2 H 2 2 mol C 2 H 2 1 mol H 2 O = 36.0g H 2 O b) How many grams O 2 to burn 52.0g C 2 H 2 ? c) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O

14 Ch12 HW# ) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O a) How many grams of CO 2 & H 2 O are produced when 52.0g C 2 H 2 burn? CO 2 : 52.0g C 2 H 2 1 mol C 2 H 2 4 mol CO g CO g C 2 H 2 2 mol C 2 H 2 1 mol CO 2 = 176 g CO 2 H 2 O: 52.0g C 2 H 2 1 mol C 2 H 2 2 mol H 2 O 18.0g H 2 O 26.0 g C 2 H 2 2 mol C 2 H 2 1 mol H 2 O = 36.0g H 2 O b) How many grams O 2 to burn 52.0g C 2 H 2 ? 52.0g C 2 H 2 1 mol C 2 H 2 5 mol O g O g C 2 H 2 2 mol C 2 H 2 1 mol O 2 = 160g O 2 c) 2 C 2 H 2(g) + 5 O 2(g) 4 CO 2(g) + 2 H 2 O 52.0g + 160g = 176g + 36g

15 Ch12 HW# ) Aluminum reacts with HCl to produce aluminum chloride ( AlCl 3 ) and hydrogen gas. Write a balanced equation for the reaction and calculate the number of moles of HCl required to react with 0.87mol of Al. 5) Glucose (C 6 H 12 O 6 ) combines with O 2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O 2 are required to combine with 0.25mol of glucose?

16 Ch12 HW# ) Aluminum reacts with HCl to produce aluminum chloride (AlCl 3 ) and hydrogen gas. Write a balanced equation for the reaction and calculate the number of moles of HCl required to react with 0.87mol of Al. 2 Al + 6 HCl 2 AlCl H 2.87mol ?mol.87mol Al 6mol HCl 2mol Al = 2.6mol HCl 5) Glucose ( C 6 H 12 O 6 ) combines with O 2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O 2 are required to combine with 0.25mol of glucose?

17 Ch12 HW# ) Aluminum reacts with HCl to produce aluminum chloride (AlCl 3 ) and hydrogen gas. Write a balanced equation for the reaction and calculate the number of moles of HCl required to react with 0.87mol of Al. 2 Al + 6 HCl 2 AlCl H 2.87mol ?mol.87mol Al 6mol HCl 2mol Al = 2.6mol HCl 5) Glucose (C 6 H 12 O 6 ) combines with O 2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O 2 are required to combine with 0.25mol of glucose? C 6 H 12 O O 2 6 CO H 2 O.25mol ?mol.25mol C 6 H 12 O 6 6molHCl 1mol CHO = 1.5mol O 2

18 6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation: Li 3 N + 3 H 2 ONH LiOH 7) What mass of sodium chloride is produced when chloride reacts with.029g of sodium iodine?

19 6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation: Li 3 N + 3 H 2 ONH LiOH.38g Li 3 N 1mol Li 3 N 3mol LiOH 24.0g LiOH 35.0g Li 3 N 1mol Li 3 N 1mol LiOH =.78g LiOH 7) What mass of sodium chloride is produced when chloride reacts with.029g of sodium iodine?

20 6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation: Li 3 N + 3 H 2 ONH LiOH.38g Li 3 N 1mol Li 3 N 3mol LiOH 24.0g LiOH 35.0g Li 3 N 1mol Li 3 N 1mol LiOH =.78g LiOH 7) What mass of sodium chloride is produced when chloride reacts with.029g of sodium iodine? Cl Na I 2 NaCl + I 2.29g Na I 1 mol Na I 2 mol NaCl 58.5g NaCl 150.0g Na I 2 mol Na I 1 mol NaCl =.112g NaCl

21 8) Determine the mass of carbon dioxide produced when 0.85g of butane Reacts with oxygen according to : 2 C 4 H O 2 8 CO H 2 O 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb 2 O C 2 Sb + 3 CO

22 8) Determine the mass of carbon dioxide produced when 0.85g of butane Reacts with oxygen according to : 2 C 4 H O 2 8 CO H 2 O 0.85g C 4 H 10 1mol C 4 H 10 8mol CO g CO g C 4 H 10 2mol C 4 H 10 1mol CO 2 = _____g CO 2 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb 2 O C 2 Sb + 3 CO

23 8) Determine the mass of carbon dioxide produced when 0.85g of butane Reacts with oxygen according to : 2 C 4 H O 2 8 CO H 2 O 0.85g C 4 H 10 1mol C 4 H 10 8mol CO g CO g C 4 H 10 2mol C 4 H 10 1mol CO 2 = _____g CO 2 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb 2 O C 2 Sb + 3 CO.46g Sb 2 O 3 1 mol Sb 2 O 3 2 mol Sb 121.8g Sb 291.6g Sb 2 O 3 1 mol Sb 2 O 3 1 mol Sb =.38g Sb

24 10) What mass of hydrogen peroxide (H 2 O 2 ) must decompose to produce 0.77g of water? H 2 O 2  H 2 O + O 2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide?

25 10) What mass of hydrogen peroxide (H 2 O 2 ) must decompose to produce 0.77g of water? H 2 O 2  H 2 O + O g H 2 O 1 mol H 2 O 2 mol H 2 O g H 2 O g H 2 O 2 mol H 2 O 1 mol H 2 O 2 = ____g H 2 O 2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide?

26 10) What mass of hydrogen peroxide (H 2 O 2 ) must decompose to produce 0.77g of water? H 2 O 2  H 2 O + O g H 2 O 1 mol H 2 O 2 mol H 2 O g H 2 O g H 2 O 2 mol H 2 O 1 mol H 2 O 2 = ____g H 2 O 2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide? CO + O 2  CO CO 2 1 mol CO 2 2 mol CO 28.0g CO 44.0g CO 2 2 mol CO 2 1 mol CO = 0.44g CO

27 12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC 2 + H 2 O Ca(OH) 2 + C 2 H 2 13) How many grams of ozone (O 3 ) must produce 0.87g of oxygen? __O 3 __O 2

28 12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC H 2 O Ca(OH) 2 + C 2 H 2.64g H 2 O 1 mol H 2 O 1 mol Ca(OH) g Ca(OH) g H 2 O 2 mol H 2 O 1 mol Ca(OH) 2 = 1.32g Ca(OH) 2 13) How many grams of ozone (O 3 ) must produce 0.87g of oxygen? __O 3 __O 2

29 12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC H 2 O Ca(OH) 2 + C 2 H 2.64g H 2 O 1 mol H 2 O 1 mol Ca(OH) g Ca(OH) g H 2 O 2 mol H 2 O 1 mol Ca(OH) 2 = 1.32g Ca(OH) 2 13) How many grams of ozone (O 3 ) must produce 0.87g of oxygen? 2 O 3 3 O 2.87g O 2 1 mol O 2 2 mol O g O g O 2 3 mol O 2 1 mol O 3 =.87g O 3

30 Ch12.3 – More Stoichiometry Ex1) How many molecules of oxygen are produced when 29.2g of water is decomposed? Ex2) Assuming STP, how many liters of oxygen are needed to produce 19.8 L of SO 3 ? Ex3) How many mls of nitrogen dioxide are produced when 3.4 ml of oxygen react with an excess of nitrogen monoxide? Assume STP.

31 Ch12.3 – More Stoichiometry Ex1) How many molecules of oxygen are produced when 29.2g of water is decomposed? 2 H 2 O 2 H 2(g) + O 2(g) Ex2) Assuming STP, how many liters of oxygen are needed to produce 19.8 L of SO 3 ? 2 SO 2 + O 2 2 SO 3 Ex3) How many mls of nitrogen dioxide are produced when 3.4 ml of oxygen react with an excess of nitrogen monoxide? Assume STP. O NO 2 NO 2 Ch12 HW#3 14

32 Lab 12.1 Quantitative Analysis Data Analysis 1) Mass of Fe lost by nails: Δmass = Fe(before) – Fe(after) = ____ g Fe 2) Moles of Fe: Δmass of Fe = g Fe 1 mole Fe 55.8g Fe = ___ mol Fe 3) Mass of Cu produced: (mass of beaker + product) – (mass of beaker) = ___ g Cu 4) Moles of Cu: Mass Cu produced = g Cu 1 mol Cu 63.5 g Cu = ___ mol Cu 5) Mole Ratio: ___ mol Fe ___ mol Cu ___Fe + ___CuCl 2  ___FeCl 3 + ___Cu

33 Lab12.1 – Mass – Mass Conversions - lab due in 2 days - Ch12 HW#3 due at beginning of period

34 Ch12 HW#3 14 Sn (s) + 2 HF (g) SnF 2 + H 2(g) a) ? L 9.40 L b) 20.0 L ? molecules c) 7.42x10 24 molecules ?g a) b) c)

35 Ch12 HW#3 14 Sn (s) + 2 HF (g) SnF 2 + H 2(g) a) ? L 9.40 L b) 20.0 L ? molecules c) 7.42x10 24 molecules ?g a)9.40L H 2 1 mol H 2 2 mol HF 22.4L HF 22.4L H 2 1 mol H 2 1 mol HF= 18.8L b) c)

36 Ch12 HW#3 14 Sn (s) + 2 HF (g) SnF 2 + H 2(g) a) ? L 9.40 L b) 20.0 L ? molecules c) 7.42x10 24 molecules ?g a)9.40L H 2 1 mol H 2 2 mol HF 22.4L HF 22.4L H 2 1 mol H 2 1 mol HF= 18.8L b)20.0 L HF 1 mol HF 1 mol H x10 23 molecules H L HF 2 mol HF 1 mol H 2 = 2.69x10 23 molecules c)

37 Ch12 HW#3 14 Sn (s) + 2 HF (g) SnF 2 + H 2(g) a) ? L 9.40 L b) 20.0 L ? molecules c) 7.42x10 24 molecules ?g a)9.40L H 2 1 mol H 2 2 mol HF 22.4L HF 22.4L H 2 1 mol H 2 1 mol HF= 18.8L b)20.0 L HF 1 mol HF 1 mol H x10 23 molecules H L HF 2 mol HF 1 mol H 2 = 2.69x10 23 molecules c)7.42x10 24 molecules HF 1 mol HF 1 mol SnF g SnF x mol HF 1 mol SnF 2 molecules HF = 967g SnF 2

38 Ch12 HW#4 15 – g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. How many liters would the hydrogen gas occupy at STP? 16. If 30.2 of aluminum react with HCL to produce aluminum chloride and hydrogen gas, how many liters of hydrogen are produced at STP?

39 Ch12 HW#4 15 – g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. How many liters would the hydrogen gas occupy at STP? K + H 2 O KOH + H If 30.2 of aluminum react with HCL to produce aluminum chloride and hydrogen gas, how many liters of hydrogen are produced at STP? Al + HCl AlCl H 2

40 17. How many liters of HCL are produced by the reaction of 5.7L of hydrogen with an equal amount of chlorine? 18. How many liters of hydrogen are required to react with 0.45 mol of oxygen to produce water?

41 17. How many liters of HCL are produced by the reaction of 5.7L of hydrogen with an equal amount of chlorine? H 2 + Cl 2 HCl 18. How many liters of hydrogen are required to react with 0.45 mol of oxygen to produce water? H 2 + O 2 H 2 O Ch12 HW#4 19,20 for HW

42 19. How many liters of SO 2 are produced from the reaction of sulfur with 26.9L of oxygen? S + O 2 SO How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn + Cl 2 ZnCl 2

43 19. How many liters of SO 2 are produced from the reaction of sulfur with 26.9L of oxygen? S + O 2 SO L O 2 1 mol O 2 1 mol SO L SO L O 2 1 mol O 2 1 mol SO 2 = 26.9L SO How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn + Cl 2 ZnCl 2

44 19. How many liters of SO 2 are produced from the reaction of sulfur with 26.9L of oxygen? S + O 2 SO L O 2 1 mol O 2 1 mol SO L SO L O 2 1 mol O 2 1 mol SO 2 = 26.9L SO How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn + Cl 2 ZnCl L Cl 2 1 mol Cl 2 1 mol ZnCl g ZnCl L Cl 2 1 mol Cl 2 1 mol ZnCl 2 = 102.3g ZnCl 2

45 Ch12 Mid Chapter Review 1. In Lab12.1 you reacted 2 iron nails with copper (II) chloride. If the nails massed at 4.25g, and there was enough CuCl 2 to completely dissolve the nails, what mass of copper would be produced? ___Fe + ___CuCl 2  ___Cu + ___FeCl 3 2. In ch11, magnesium reacted with carbon dioxide to produce magnesium oxide, carbon, and lots of bright light! How many molecules of carbon dioxide are required to react with 2.50g of Mg?

46 3. If lead wasn’t so dangerous for the environment, we would decompose 3.00g of PbCO 3. Pb(OH) 2 to obtain CO 2. What volume should be produced? 2 PbCO 3. Pb(OH) 2  3PbO + H 2 O + 2 CO 2

47 Ch12 MCR HW 1 – 3 1. If only 1.00g of the iron nails actually dissolved, what mass of copper would be produced? 2 Fe + 3 CuCl 2 2 FeCl Cu 2. How many molecules of carbon dioxide are required to react with 12.04x10 23 atoms of Mg? 2 Mg + CO 2 2 MgO + C

48 Ch12 MCR HW 1 – 3 1. If only 1.00g of the iron nails actually dissolved, what mass of copper would be produced? 2 Fe + 3 CuCl 2 2 FeCl Cu 1.00g Fe 1 mol Fe3 mol Cu 63.5g Cu 55.8g Fe2 mol Fe 1 mol Cu= 1.17g Cu 2. How many molecules of carbon dioxide are required to react with 12.04x10 23 atoms of Mg? 2 Mg + CO 2 2 MgO + C

49 Ch12 MCR HW 1 – 3 1. If only 1.00g of the iron nails actually dissolved, what mass of copper would be produced? 2 Fe + 3 CuCl 2 2 FeCl Cu 1.00g Fe 1 mol Fe3 mol Cu 63.5g Cu 55.8g Fe2 mol Fe 1 mol Cu= 1.17g Cu 2. How many molecules of carbon dioxide are required to react with 12.04x10 23 atoms of Mg? 2 Mg + CO 2 2 MgO + C 12.04x x10 23 atoms Mg 1 mol Mg1 mol CO 2 molecules CO x mol CO 2 1 mol CO 2 = 6.02x10 23 atoms Mg molecules CO 2

50 3. What volumes of CO 2 should be produced if 4.00 g of lead carbonate decompose? 2PbCO 3 Pb(OH) 3 3 PbO + H 2 O + 2 CO 2

51 3. What volumes of CO 2 should be produced if 4.00 g of lead carbonate decompose? 2PbCO 3 Pb(OH) 3 3 PbO + H 2 O + 2 CO g 2PbCO 3 1 mol 2PbCO 3 2 mol Co L CO g 2PbCO 3 1 mol 2PbCO 3 1 mol CO 2 = 0.23L

52 Ch12.5 – Limiting Reactants Cookie recipe: To make 1 dozen cookies, need 2 eggs, 1 cup sugar. I have 10 eggs and 3 cups of sugar, how many dozens? Ex 1) What is the max # of grams of Cu 2 S that can be formed when 80.0g of Cu react with 25.0g of S? And, which of them was the limiting reactant? 2 Cu + S Cu 2 S

53 Ch12.5 – Limiting Reactants Cookie recipe: To make 1 dozen cookies, need 2 eggs, 1 cup sugar. I have 10 eggs and 3 cups of sugar, how many dozens? Ex 1) What is the max # of grams of Cu 2 S that can be formed when 80.0g of Cu react with 25.0g of S? And, which of them was the limiting reactant? 2 Cu + S Cu 2 S 80g 2 Sg ? g 80.0g Cu 1 mol Cu 1 mol Cu 2 S 159.1g Cu 2 S 63.5g Cu 2 mol Cu 1 mol Cu 2 S= 100.2g Cu 2 S 25.0g S 1 mol S 1 mol Cu 2 S 159.1g Cu 2 S 32.1g S 1 mol S 1 mol Cu 2 S= 124g Cu 2 S = = 32.1 Cu is the Limiting g/mol Reactant Ch12 HW#5

54 Ch12 HW#5 21. C 2 H 5 OH + O 2 CO 2 + H 2 O; 60 grams C 2 H 5 OH, 26L O 2 at STP 22. N 2 + O 2 NO; 30 grams N 2, 30 grams O 2

55 23. CO + H 2 CH 3 OH; 25 grams CO, 10.0g H 2

56 24. 2 Al + 3 I 2 AlI 3 ; grams Al, 200.0g I Ca(OH) 2 + HBr CaBr 2 + H 2 O; 80.0 grams Ca(OH) g HBr.

57 24. 2 Al + 3 I 2 AlI 3 ; grams Al, 200.0g I g Al 1 mol Al 2 mol Al I g Al I g Al 2 mol Al 1 mol Al I 3 = 2265g 200.0g I 2 1 mol I 2 2 mol Al I g Al I g I 2 3 mol I 2 1 mol Al I 3 = 213.6g I 2 is the L.R. 25. Ca(OH) 2 + HBr CaBr 2 + H 2 O; 80.0 grams Ca(OH) g HBr.

58 24. 2 Al + 3 I 2 AlI 3 ; grams Al, 200.0g I g Al 1 mol Al 2 mol Al I g Al I g Al 2 mol Al 1 mol Al I 3 = 2265g 200.0g I 2 1 mol I 2 2 mol Al I g Al I g I 2 3 mol I 2 1 mol Al I 3 = 213.6g I 2 is the L.R. 25. Ca(OH) 2 + HBr CaBr 2 + H 2 O; 80.0 grams Ca(OH) g HBr. 80.0g Ca(OH) 2 1 mol Ca(OH) 2 1 mol CaBr g CaBr g Ca(OH) 2 1 mol Ca(OH) 2 1 mol CaBr 2 = 216g 75g HBr 1 mol HBr 1 mol CaBr g CaBr g HBr 2 mol HBr 1 mol CaBr 2 = 92.7g

59 Ch12 HW# Cr + H 3 PO 4 CrPO 4 + H 2 ; given 50.0 g Cr and 35.0g H 3 PO 4, how many grams of H 2 will be produced? 27. C 6 H 14 + O 2 CO 2 + H 2 O; given 75 grams C 6 H 14 and 35.2 L O 2 at STP, how many liters of CO 2 will be produced?

60 Ch12 HW# Cr + H 3 PO 4 CrPO 4 + H 2 ; given 50.0 g Cr and 35.0g H 3 PO 4, how many grams of H 2 will be produced? 50g Cr 1 mol Cr 3 mol H 2 2.0g H g Cr 2 mol Cr 1 mol H 2 = 2.8g H 2 35g H 3 PO 4 1 mol H 3 PO 4 3 mol H 2 2.0g H g H 3 PO 4 2 mol H 3 PO 4 1 mol H 2 = 1.0g H C 6 H 14 + O 2 CO 2 + H 2 O; given 75 grams C 6 H 14 and 35.2 L O 2 at STP, how many liters of CO 2 will be produced?

61 Ch12 HW# Cr + H 3 PO 4 CrPO 4 + H 2 ; given 50.0 g Cr and 35.0g H 3 PO 4, how many grams of H 2 will be produced? 50g Cr 1 mol Cr 3 mol H 2 2.0g H g Cr 2 mol Cr 1 mol H 2 = 2.8g H 2 35g H 3 PO 4 1 mol H 3 PO 4 3 mol H 2 2.0g H g H 3 PO 4 2 mol H 3 PO 4 1 mol H 2 = 1.0g H C 6 H 14 + O 2 CO 2 + H 2 O; given 75 grams C 6 H 14 and 35.2 L O 2 at STP, how many liters of CO 2 will be produced? 75g C 6 H 14 1 mol C 6 H mol CO L CO g C 6 H 14 2 mol C 6 H 14 1 mol CO 2 = L CO L O 2 1 mol O 2 12mol CO L CO L O 2 19 mol O 2 1 mol CO 2 =22.2 L CO 2

62 28) When 65.14g of CaCl 2 reacts with 74.68g of NA 2 CO 3, they produce CaCO 3 and how many grams of NaCl? CaCl 2 + Na 2 CO 3  CaCO 3 + NaCl 29) If 4.1g of Cr is heated with 9.3g of Cl 2 what mass of CrCl 3 will be produced? Cr + Cl 2  CrCl 3

63 28) When 65.14g of CaCl 2 reacts with 74.68g of NA 2 CO 3, they produce CaCO 3 and how many grams of NaCl? CaCl 2 + Na 2 CO 3  CaCO 3 + NaCl 65.14g CaCl 2 1 mol CaCl 2 2 mol NaCl 58.5 g NaCl 111.1g CaCl 2 1 mol CaCl 2 1 mol NaCl =68.6g NaCl 74.68g Na 2 CO 3 1 mol Na 2 CO 3 2 mol NaCl 58.5 g NaCl 106.0g Na 2 CO 3 1 mol Na 2 CO 3 1 mol NaCl = 82.5g NaCl 29) If 4.1g of Cr is heated with 9.3g of Cl 2 what mass of CrCl 3 will be produced? Cr + Cl 2  CrCl 3

64 28) When 65.14g of CaCl 2 reacts with 74.68g of NA 2 CO 3, they produce CaCO 3 and how many grams of NaCl? CaCl 2 + Na 2 CO 3  CaCO 3 + NaCl 65.14g CaCl 2 1 mol CaCl 2 2 mol NaCl 58.5 g NaCl 111.1g CaCl 2 1 mol CaCl 2 1 mol NaCl =68.6g NaCl 74.68g Na 2 CO 3 1 mol Na 2 CO 3 2 mol NaCl 58.5 g NaCl 106.0g Na 2 CO 3 1 mol Na 2 CO 3 1 mol NaCl = 82.5g NaCl 29) If 4.1g of Cr is heated with 9.3g of Cl 2 what mass of CrCl 3 will be produced? Cr + Cl 2  CrCl 3 4.1g Cr 1 mol Cr 2 mol CrCl g CrCl g Cr 2 mol Cr 1 mol CrCl 3 = 12.5g CrCl 3 9.3g Cl 2 1 mol Cl 2 2 mol CrCl g CrCl g Cl 2 3 mol Cl 2 1 mol CrCl 3 = 13.9 g CrCl 3

65 Ch12 Rev 1) Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur dioxide. __C + __SO 2 __CS 2 +__CO How many moles of CS 2 form when 2.7 moles of C react? 2) Methanol, CH 3 OH, is used in the production of many chemicals. It is made by reacting carbon monoxide and hydrogen at high temps and pressure. How many moles of carbon monoxide are needed to produce 360 g CH 3 OH? CO + 2H 2 CH 3 OH

66 3) The reaction of fluorine with ammonia produces dinitrogen tetrafluoride and hydrogen fluoride. If you have 66.6 g of NH 3, how many grams of F 2 are required to complete the reaction? 5 F 2 + 2NH 3 N 2 F HF 4) Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. 4 Zn + 10 HNO 3 4 Zn(NO 3 ) 2 + NH 4 NO H 2 O How many atoms of zinc react with 1.49 g of HNO 3 ?

67 6. Ammononium nitrate decomposes explosively at high temps to form nitrogen, oxygen, and water vapor. What is the total number of liters of O 2 gas formed when 228g of NH 4 NO 3 is decomposed? NH 4 NO 3  2N 2 + 4H 2 O + O 2 7. If 100g of carbon reacts with 85.0g of B 2 O 3, how many grams of B 4 C 3 will be produced?___B 2 O 3 + ___C  ___B 4 C 3 + ___CO 2


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