# Ch12.1 - Stoichiometry N2(g) + H2(g) NH3(g)

## Presentation on theme: "Ch12.1 - Stoichiometry N2(g) + H2(g) NH3(g)"— Presentation transcript:

Ch Stoichiometry N2(g) H2(g) NH3(g)

Ch Stoichiometry 1N2(g) H2(g) NH3(g) 1 mole reacts with 3 moles to produce 2 moles Masses: = 28.0 g/mol = g/mol = 14.0 = 3.0 17.0 g/mol How many moles of NH3 produced? - 2 mol of N2 react? - 1½ mol of H2 react? - 28 g of N2 react?

Ex1) Calculate the # of moles of nitrogen required
to make 7.24 moles of ammonia. N H NH3 HW#1) Given 4 Al O Al2O3 How many moles of Al are needed to form 3.7 mol of Al2O3? b) How many moles of O2 are required to react completely with 14.8 moles of Al?

Ex1) Calculate the # of moles of nitrogen required
to make 7.24 moles of ammonia. N H NH3 ? moles moles 7.24 moles NH moles N2 2moles NH3 = 3.62 moles N2 HW#1) Given 4 Al O Al2O3 ? Mol mol How many moles of Al are needed to form 3.7 mol of Al2O3? 3.7 mol Al2O mol Al 2 mol Al2O3 = 7.4 mol Al b) How many moles of O2 are required to react completely with 14.8 moles of Al? 14.8 mol Al 3 mol O2 4 mol Al = 11.1 mol O2

Mass – Mass Calcs Ex2) Calculate the # of grams of NH3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. N2(g) H2(g) NH3(g) Ex3) How many grams of nitrogen are needed to produce the 30.6g of NH3 needed for the reaction? N2(g) H2(g) NH3(g)

Mass – Mass Calcs Ex2) Calculate the # of grams of NH3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. N2(g) H2(g) NH3(g) 5.40 H2 1 mol H2 2 mol NH g NH3 2.0 g H mol H mol NH3 = 30.6g NH3 Ex3) How many grams of nitrogen are needed to produce the 30.6g of NH3 needed for the reaction? N2(g) H2(g) NH3(g) 30.6g NH3 1 mol NH mol N g N2 17.0 g NH3 2 mol NH3 1 mol N = 25.2g N2

HW#2) CaC2(s) + H2O C2H2(g) + Ca(OH)2(aq)
a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced?

HW#2) 1CaC2(s) + 2H2O 1C2H2(g) + 1Ca(OH)2(aq)
a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? 49.0g H2O 1 mol H2O mol CaC2 18.0g H2O mol H2O = 1.36 moles CaC2 b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced?

HW#2) 1CaC2(s) + 2H2O 1C2H2(g) + 1Ca(OH)2(aq)
a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? 49.0g H2O 1 mol H2O mol CaC2 18.0g H2O mol H2O = 1.36 moles CaC2 b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? 5.00g CaC2 1 mol CaC mol C2H g C2H2 52.1g CaC mol CaC2 1 mol C2H2 = 2.49g C2H2 c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced? CH 12 HW#1 1-3

HW#2) 1CaC2(s) + 2H2O 1C2H2(g) + 1Ca(OH)2(aq)
a. How many moles of CaC2 are needed to react completely with 49.0g of H2O? 49.0g H2O 1 mol H2O mol CaC2 18.0g H2O mol H2O = 1.36 moles CaC2 b. How many grams of Ca(OH)2 are produced by 5.00g of CaC2? 5.00g CaC2 1 mol CaC mol C2H g C2H2 52.1g CaC mol CaC2 1 mol C2H2 = 2.49g C2H2 c. How many grams of Ca(OH)2 are produced when 0.89 mol of C2H2 are produced? .89 mol C2H2 1 mol Ca(OH) g Ca(OH)2 1 mol C2H mol Ca(OH)2 = 66.0g Ca(OH)2 CH 12 HW#1 1-3

Ch12 HW#1 1-3 3) 2 C2H2(g) O2(g) CO2(g) H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : H2O: b) How many grams O2 to burn 52.0g C2H2? c) 2 C2H2(g) O2(g) CO2(g) H2O

Ch12 HW#1 1-3 3) 2 C2H2(g) O2(g) CO2(g) H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : 52.0g C2H2 1 mol C2H2 4 mol CO g CO g C2H2 2 mol C2H mol CO = 176 g CO2 H2O: b) How many grams O2 to burn 52.0g C2H2? c) 2 C2H2(g) O2(g) CO2(g) H2O

Ch12 HW#1 1-3 3) 2 C2H2(g) O2(g) CO2(g) H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : 52.0g C2H2 1 mol C2H2 4 mol CO g CO g C2H2 2 mol C2H mol CO = 176 g CO2 H2O: 52.0g C2H2 1 mol C2H2 2 mol H2O g H2O g C2H2 2 mol C2H mol H2O = 36.0g H2O b) How many grams O2 to burn 52.0g C2H2? c) 2 C2H2(g) O2(g) CO2(g) H2O

Ch12 HW#1 1-3 3) 2 C2H2(g) O2(g) CO2(g) H2O a) How many grams of CO2 & H2O are produced when 52.0g C2H2 burn? CO2 : 52.0g C2H2 1 mol C2H2 4 mol CO g CO g C2H2 2 mol C2H mol CO = 176 g CO2 H2O: 52.0g C2H2 1 mol C2H2 2 mol H2O g H2O g C2H2 2 mol C2H mol H2O = 36.0g H2O b) How many grams O2 to burn 52.0g C2H2? 52.0g C2H2 1 mol C2H2 5 mol O g O g C2H2 2 mol C2H2 1 mol O = 160g O2 c) 2 C2H2(g) O2(g) CO2(g) H2O 52.0g g = g g

Ch12 HW#2 4-13 4) Aluminum reacts with HCl to produce aluminum chloride (AlCl3) 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 (C6H12O6) combines with O2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O2 are required to combine with 0.25mol of glucose?

2 Al + 6 HCl 2 AlCl3 + 3 H2 .87mol ?mol .87mol Al 6mol HCl
Ch12 HW#2 4-13 4) Aluminum reacts with HCl to produce aluminum chloride (AlCl3) 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 AlCl3 + 3 H2 .87mol ?mol .87mol Al 6mol HCl 2mol Al = 2.6mol HCl 5) Glucose (C6H12O6) combines with O2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O2 are required to combine with 0.25mol of glucose?

2 Al + 6 HCl 2 AlCl3 + 3 H2 .87mol ?mol .87mol Al 6mol HCl
Ch12 HW#2 4-13 4) Aluminum reacts with HCl to produce aluminum chloride (AlCl3) 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 AlCl3 + 3 H2 .87mol ?mol .87mol Al 6mol HCl 2mol Al = 2.6mol HCl 5) Glucose (C6H12O6) combines with O2 in the body to produce carbon dioxide and water. Write a balanced equation for this reaction. How many moles of O2 are required to combine with 0.25mol of glucose? C6H12O O2 6 CO H2O .25mol ?mol .25mol C6H12O6 6molHCl 1mol CHO = 1.5mol O2

6) Determine the mass of lithium hydroxide produced when 0
6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation: Li3N + 3 H2O NH LiOH 7) What mass of sodium chloride is produced when chloride reacts with .029g of sodium iodine?

.38g Li3N 1mol Li3N 3mol LiOH 24.0g LiOH
6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation: Li3N + 3 H2O NH LiOH .38g Li3N 1mol Li3N 3mol LiOH 24.0g LiOH 35.0g Li3N 1mol Li3N 1mol LiOH = .78g LiOH 7) What mass of sodium chloride is produced when chloride reacts with .029g of sodium iodine?

.38g Li3N 1mol Li3N 3mol LiOH 24.0g LiOH
6) Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation: Li3N + 3 H2O NH LiOH .38g Li3N 1mol Li3N 3mol LiOH 24.0g LiOH 35.0g Li3N 1mol Li3N 1mol LiOH = .78g LiOH 7) What mass of sodium chloride is produced when chloride reacts with .029g of sodium iodine? Cl2 + 2 NaI NaCl + I2 .29g NaI 1 mol NaI mol NaCl g NaCl 150.0g NaI 2 mol NaI mol NaCl = .112g NaCl

8) Determine the mass of carbon dioxide produced when 0.85g of butane
Reacts with oxygen according to : 2 C4H O CO H2O 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb2O C Sb + 3 CO

8) Determine the mass of carbon dioxide produced when 0.85g of butane
Reacts with oxygen according to : 2 C4H O CO H2O 0.85g C4H10 1mol C4H10 8mol CO g CO2 58.0g C4H10 2mol C4H10 1mol CO2 = _____g CO2 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb2O C Sb + 3 CO

8) Determine the mass of carbon dioxide produced when 0.85g of butane
Reacts with oxygen according to : 2 C4H O CO H2O 0.85g C4H10 1mol C4H10 8mol CO g CO2 58.0g C4H10 2mol C4H10 1mol CO2 = _____g CO2 9) Determine the mass of antimony produced when 0.46g of antimony (III) oxide reacts with carbon according to the following equation: Sb2O C Sb + 3 CO .46g Sb2O3 1 mol Sb2O3 2 mol Sb g Sb 291.6g Sb2O3 1 mol Sb2O3 1 mol Sb = .38g Sb

10) What mass of hydrogen peroxide (H2O2) must decompose to produce
0.77g of water? H2O2  H2O O2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide?

H2O2  H2O + O2 0.77g H2O 1 mol H2O 2 mol H2O2 34.0g H2O2
10) What mass of hydrogen peroxide (H2O2) must decompose to produce 0.77g of water? H2O2  H2O O2 0.77g H2O 1 mol H2O 2 mol H2O g H2O2 18.0g H2O 2 mol H2O 1 mol H2O = ____g H2O2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide?

CO + O2  CO2 0.69 CO2 1 mol CO2 2 mol CO 28.0g CO
10) What mass of hydrogen peroxide (H2O2) must decompose to produce 0.77g of water? H2O2  H2O O2 0.77g H2O 1 mol H2O 2 mol H2O g H2O2 18.0g H2O 2 mol H2O 1 mol H2O = ____g H2O2 11) What mass of carbon monoxide must react with oxygen to produce 0.69g of carbon dioxide? CO O2  CO2 0.69 CO2 1 mol CO mol CO g CO 44.0g CO mol CO mol CO = 0.44g CO

CaC2 + H2O Ca(OH)2 + C2H2 __O3 __O2
12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC H2O Ca(OH) C2H2 13) How many grams of ozone (O3) must produce 0.87g of oxygen? __O __O2

.64g H2O 1 mol H2O 1 mol Ca(OH)2 74.1g Ca(OH)2
12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC H2O Ca(OH) C2H2 .64g H2O 1 mol H2O 1 mol Ca(OH) g Ca(OH)2 18.0 g H2O 2 mol H2O mol Ca(OH)2 = 1.32g Ca(OH)2 13) How many grams of ozone (O3) must produce 0.87g of oxygen? __O __O2

.64g H2O 1 mol H2O 1 mol Ca(OH)2 74.1g Ca(OH)2
12) Determine the mass of calcium hydroxide produced when calcium carbide reacts with 3.64g of water according to the following equation: CaC H2O Ca(OH) C2H2 .64g H2O 1 mol H2O 1 mol Ca(OH) g Ca(OH)2 18.0 g H2O 2 mol H2O mol Ca(OH)2 = 1.32g Ca(OH)2 13) How many grams of ozone (O3) must produce 0.87g of oxygen? 2 O O2 .87g O mol O mol O g O3 32.0g O mol O mol O3 = .87g O3

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 SO3? Ex3) How many mls of nitrogen dioxide are produced when 3.4 ml of oxygen react with an excess of nitrogen monoxide? Assume STP.

Ch12 HW#3 14 Ch12.3 – More Stoichiometry
Ex1) How many molecules of oxygen are produced when 29.2g of water is decomposed? 2 H2O H2(g) + O2(g) Ex2) Assuming STP, how many liters of oxygen are needed to produce 19.8 L of SO3? 2 SO2 + O SO3 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 NO2 Ch12 HW#3 14

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 + ___CuCl2  ___FeCl3 + ___Cu

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

a) b) c) Ch12 HW#3 14 Sn(s) + 2 HF(g) SnF2 + H2(g) a) ? L 9.40 L
b) L ? molecules c) x1024 molecules ?g a) b) c)

9.40L H2 1 mol H2 2 mol HF 22.4L HF 22.4L H2 1 mol H2 1 mol HF = 18.8L
Ch12 HW#3 14 Sn(s) HF(g) SnF H2(g) a) ? L L b) L ? molecules c) x1024 molecules ?g 9.40L H2 1 mol H mol HF 22.4L HF 22.4L H mol H mol HF = 18.8L b) c)

20.0 L HF 1 mol HF 1 mol H2 6.02x1023 molecules H2
Ch12 HW#3 14 Sn(s) HF(g) SnF H2(g) a) ? L L b) L ? molecules c) x1024 molecules ?g 9.40L H2 1 mol H mol HF 22.4L HF 22.4L H mol H mol HF = 18.8L 20.0 L HF 1 mol HF mol H x1023 molecules H2 22.4L HF mol HF 1 mol H2 = 2.69x1023 molecules c)

20.0 L HF 1 mol HF 1 mol H2 6.02x1023 molecules H2
Ch12 HW#3 14 Sn(s) HF(g) SnF H2(g) a) ? L L b) L ? molecules c) x1024 molecules ?g 9.40L H2 1 mol H mol HF 22.4L HF 22.4L H mol H mol HF = 18.8L 20.0 L HF 1 mol HF mol H x1023 molecules H2 22.4L HF mol HF 1 mol H2 = 2.69x1023 molecules 7.42x1024 molecules HF 1 mol HF 1 mol SnF g SnF2 6.02x mol HF mol SnF2 molecules HF = 967g SnF2

Ch12 HW#4 15 – 20 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?

Ch12 HW#4 15 – 20 g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. How many liters would the hydrogen gas occupy at STP? K H2O KOH H2 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? Al HCl AlCl H2

17. How many liters of HCL are produced by the reaction of 5
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?

17. How many liters of HCL are produced by the reaction of 5
17. How many liters of HCL are produced by the reaction of 5.7L of hydrogen with an equal amount of chlorine? H Cl HCl 18. How many liters of hydrogen are required to react with 0.45 mol of oxygen to produce water? H O H2O Ch12 HW#4 19,20 for HW

19. How many liters of SO2 are produced from the reaction of sulfur
with 26.9L of oxygen? S O SO2 20. How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn Cl ZnCl2

19. How many liters of SO2 are produced from the reaction of sulfur
with 26.9L of oxygen? S O SO2 26.9L O mol O mol SO L SO2 22.4L O2 1 mol O mol SO2 = 26.9L SO2 20. How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn Cl ZnCl2

16.8L Cl2 1 mol Cl2 1 mol ZnCl2 136.4g ZnCl2
19. How many liters of SO2 are produced from the reaction of sulfur with 26.9L of oxygen? S O SO2 26.9L O mol O mol SO L SO2 22.4L O2 1 mol O mol SO2 = 26.9L SO2 20. How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8L of chlorine at STP? Zn Cl ZnCl2 16.8L Cl2 1 mol Cl2 1 mol ZnCl g ZnCl2 22.4L Cl2 1 mol Cl mol ZnCl = 102.3g ZnCl2

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 CuCl2 to completely dissolve the nails, what mass of copper would be produced? ___Fe + ___CuCl2  ___Cu + ___FeCl3 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?

3. If lead wasn’t so dangerous for the environment, we would decompose
3.00g of PbCO3.Pb(OH)2 to obtain CO2. What volume should be produced? 2 PbCO3.Pb(OH)2  3PbO + H2O + 2 CO2

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 CuCl FeCl Cu 2. How many molecules of carbon dioxide are required to react with 12.04x1023 atoms of Mg? 2 Mg CO MgO C

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 CuCl FeCl Cu 1.00g Fe 1 mol Fe 3 mol Cu g Cu 55.8g Fe 2 mol Fe 1 mol Cu = 1.17g Cu 2. How many molecules of carbon dioxide are required to react with 12.04x1023 atoms of Mg? 2 Mg CO MgO C

atoms Mg 1 mol Mg 1 mol CO2 molecules CO2
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 CuCl FeCl Cu 1.00g Fe 1 mol Fe 3 mol Cu g Cu 55.8g Fe 2 mol Fe 1 mol Cu = 1.17g Cu 2. How many molecules of carbon dioxide are required to react with 12.04x1023 atoms of Mg? 2 Mg CO MgO C 12.04x x1023 atoms Mg 1 mol Mg 1 mol CO2 molecules CO2 6.02x mol CO2 1 mol CO = 6.02x1023 atoms Mg molecules CO2

3. What volumes of CO2 should be produced if 4
3. What volumes of CO2 should be produced if 4.00 g of lead carbonate decompose? 2PbCO3 Pb(OH) PbO H2O CO2

4.00g 2PbCO3 1 mol 2PbCO3 2 mol Co2 22.4L CO2
3. What volumes of CO2 should be produced if 4.00 g of lead carbonate decompose? 2PbCO3 Pb(OH) PbO H2O CO2 4.00g 2PbCO3 1 mol 2PbCO mol Co L CO2 775.6g 2PbCO3 1 mol 2PbCO3 1 mol CO2 = 0.23L

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 Cu2S 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 Cu2S

80g 2 Sg ? g 80.0g Cu 1 mol Cu 1 mol Cu2S 159.1g Cu2S
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 Cu2S 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 Cu2S 80g Sg ? g 80.0g Cu 1 mol Cu 1 mol Cu2S g Cu2S 63.5g Cu 2 mol Cu mol Cu2S = 100.2g Cu2S 25.0g S 1 mol S 1 mol Cu2S g Cu2S 32.1g S mol S 1 mol Cu2S = 124g Cu2S = 127.0 = Cu is the Limiting 159.1 g/mol Reactant Ch12 HW#5

Ch12 HW#5 21. C2H5OH + O CO2 + H2O; 60 grams C2H5OH, 26L O2 at STP 22. N2 + O NO; 30 grams N2, 30 grams O2

23. CO + H CH3OH; 25 grams CO, 10.0g H2

24. 2 Al + 3 I AlI3; grams Al, 200.0g I2. 25. Ca(OH)2 + HBr CaBr2 + H2O; 80.0 grams Ca(OH)2 75.0g HBr.

24. 2 Al + 3 I AlI3; grams Al, 200.0g I2. 150.0g Al 1 mol Al 2 mol AlI g AlI3 27.0g Al 2 mol Al mol AlI3 = 2265g 200.0g I2 1 mol I mol AlI g AlI3 253.8g I mol I mol AlI = 213.6g I2 is the L.R. 25. Ca(OH)2 + HBr CaBr2 + H2O; 80.0 grams Ca(OH)2 75.0g HBr.

24. 2 Al + 3 I AlI3; grams Al, 200.0g I2. 150.0g Al 1 mol Al 2 mol AlI g AlI3 27.0g Al 2 mol Al mol AlI3 = 2265g 200.0g I2 1 mol I mol AlI g AlI3 253.8g I mol I mol AlI = 213.6g I2 is the L.R. 25. Ca(OH)2 + HBr CaBr2 + H2O; 80.0 grams Ca(OH)2 75.0g HBr. 80.0g Ca(OH)2 1 mol Ca(OH)2 1 mol CaBr g CaBr2 74.1g Ca(OH)2 1 mol Ca(OH)2 1 mol CaBr2 = 216g 75g HBr 1 mol HBr 1 mol CaBr g CaBr2 80.9g HBr 2 mol HBr mol CaBr2 = 92.7g

Ch12 HW# 26. Cr + H3PO CrPO4 + H2; given 50.0 g Cr and 35.0g H3PO4, how many grams of H2 will be produced? 27. C6H O CO H2O; given 75 grams C6H14 and 35.2 L O2 at STP, how many liters of CO2 will be produced?

Ch12 HW# 26. Cr + H3PO CrPO4 + H2; given 50.0 g Cr and 35.0g H3PO4, how many grams of H2 will be produced? 50g Cr 1 mol Cr 3 mol H2 2.0g H2 52.0g Cr 2 mol Cr 1 mol H2 = 2.8g H2 35g H3PO mol H3PO mol H g H2 98.0g H3PO mol H3PO mol H2 = 1.0g H2 27. C6H O CO H2O; given 75 grams C6H14 and 35.2 L O2 at STP, how many liters of CO2 will be produced?

Ch12 HW# 26. Cr + H3PO CrPO4 + H2; given 50.0 g Cr and 35.0g H3PO4, how many grams of H2 will be produced? 50g Cr 1 mol Cr 3 mol H2 2.0g H2 52.0g Cr 2 mol Cr 1 mol H2 = 2.8g H2 35g H3PO mol H3PO mol H g H2 98.0g H3PO mol H3PO mol H2 = 1.0g H2 27. C6H O CO H2O; given 75 grams C6H14 and 35.2 L O2 at STP, how many liters of CO2 will be produced? 75g C6H mol C6H mol CO L CO2 86.0g C6H mol C6H mol CO2 = L CO2 35.2 L O mol O mol CO L CO2 22.4 L O mol O mol CO2 =22.2 L CO2

CaCl2 + Na2CO3  CaCO3 + NaCl Cr + Cl2  CrCl3
28) When 65.14g of CaCl2 reacts with 74.68g of NA2CO3, they produce CaCO3 and how many grams of NaCl? CaCl Na2CO3  CaCO NaCl 29) If 4.1g of Cr is heated with 9.3g of Cl2 what mass of CrCl3 will be produced? Cr + Cl2  CrCl3

65.14g CaCl2 1 mol CaCl2 2 mol NaCl 58.5 g NaCl
28) When 65.14g of CaCl2 reacts with 74.68g of NA2CO3, they produce CaCO3 and how many grams of NaCl? CaCl Na2CO3  CaCO NaCl 65.14g CaCl2 1 mol CaCl mol NaCl g NaCl 111.1g CaCl mol CaCl mol NaCl =68.6g NaCl 74.68g Na2CO mol Na2CO mol NaCl g NaCl 106.0g Na2CO mol Na2CO mol NaCl = 82.5g NaCl 29) If 4.1g of Cr is heated with 9.3g of Cl2 what mass of CrCl3 will be produced? Cr + Cl2  CrCl3

65.14g CaCl2 1 mol CaCl2 2 mol NaCl 58.5 g NaCl
28) When 65.14g of CaCl2 reacts with 74.68g of NA2CO3, they produce CaCO3 and how many grams of NaCl? CaCl Na2CO3  CaCO NaCl 65.14g CaCl2 1 mol CaCl mol NaCl g NaCl 111.1g CaCl mol CaCl mol NaCl =68.6g NaCl 74.68g Na2CO mol Na2CO mol NaCl g NaCl 106.0g Na2CO mol Na2CO mol NaCl = 82.5g NaCl 29) If 4.1g of Cr is heated with 9.3g of Cl2 what mass of CrCl3 will be produced? Cr + Cl2  CrCl3 4.1g Cr mol Cr mol CrCl g CrCl3 52.0g Cr 2 mol Cr mol CrCl3 = 12.5g CrCl3 9.3g Cl mol Cl mol CrCl g CrCl3 71.0 g Cl mol Cl mol CrCl3 = 13.9 g CrCl3

__C + __SO2 __CS2 +__CO Ch12 Rev
1) Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur dioxide. __C + __SO __CS2 +__CO How many moles of CS2 form when 2.7 moles of C react? 2) Methanol, CH3OH, 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 CH3OH? CO + 2H CH3OH

4 Zn + 10 HNO3 4 Zn(NO3)2 + NH4NO3 + 3 H2O
3) The reaction of fluorine with ammonia produces dinitrogen tetrafluoride and hydrogen fluoride. If you have 66.6 g of NH3, how many grams of F2 are required to complete the reaction? 5 F2 + 2NH N2F4 + 6 HF 4) Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. 4 Zn + 10 HNO Zn(NO3)2 + NH4NO3 + 3 H2O How many atoms of zinc react with 1.49 g of HNO3 ?

6. Ammononium nitrate decomposes explosively at high temps to form
nitrogen, oxygen, and water vapor. What is the total number of liters of O2 gas formed when 228g of NH4NO3 is decomposed? NH4NO3  2N2 + 4H2O + O2 7. If 100g of carbon reacts with 85.0g of B2O3, how many grams of B4C3 will be produced? ___B2O3 + ___C  ___B4C3 + ___CO2