Chapter 9 Stoichiometry Stoichiometry Composition stoichiometry Mass relationships
![Chapter 9 Stoichiometry Chapter 9 Stoichiometry](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-1.jpg)
![Stoichiometry • Composition stoichiometry – Mass relationships of elements in compounds • Reaction stoichiometry Stoichiometry • Composition stoichiometry – Mass relationships of elements in compounds • Reaction stoichiometry](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-2.jpg)
![Reaction Stoichiometry • Use ratios from balanced equation • Problem Type 1 – Given Reaction Stoichiometry • Use ratios from balanced equation • Problem Type 1 – Given](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-3.jpg)
![Reaction Stoichiometry • Problem Type 3 – Given in grams & unknown in moles Reaction Stoichiometry • Problem Type 3 – Given in grams & unknown in moles](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-4.jpg)
![Mole Ratio • Conversion factor that relates amount of moles of substances 2 Al Mole Ratio • Conversion factor that relates amount of moles of substances 2 Al](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-5.jpg)
![Molar Mass • The mass (in g) of 1 mole of substance 2 Al Molar Mass • The mass (in g) of 1 mole of substance 2 Al](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-6.jpg)
![Conversions • Problem Type 1 – Mole to mole – One conversion factor: mole Conversions • Problem Type 1 – Mole to mole – One conversion factor: mole](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-7.jpg)
![Conversions • In a spacecraft, the CO 2 exhaled by astronauts can be removed Conversions • In a spacecraft, the CO 2 exhaled by astronauts can be removed](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-8.jpg)
![Conversions • The disinfectant hydrogen peroxide, H 2 O 2, decomposes to form water Conversions • The disinfectant hydrogen peroxide, H 2 O 2, decomposes to form water](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-9.jpg)
![Conversions • Problem Type 2 – Mole to mass – Two conversion factors: mole Conversions • Problem Type 2 – Mole to mass – Two conversion factors: mole](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-10.jpg)
![Conversions • In photosynthesis, plants use energy from the sun to produce glucose C Conversions • In photosynthesis, plants use energy from the sun to produce glucose C](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-11.jpg)
![Conversions • What mass of CO 2, in grams, is needed to react with Conversions • What mass of CO 2, in grams, is needed to react with](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-12.jpg)
![Conversions • Problem Type 3 – Mass to moles – Two conversion factors: molar Conversions • Problem Type 3 – Mass to moles – Two conversion factors: molar](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-13.jpg)
![Conversions • The first step in the industrial manufacture of nitric acid is the Conversions • The first step in the industrial manufacture of nitric acid is the](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-14.jpg)
![Conversions • The compound Pt. Cl 2(NH 3)2 is effective as a treatment for Conversions • The compound Pt. Cl 2(NH 3)2 is effective as a treatment for](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-15.jpg)
![Conversions • Problem Type 4 – Mass to mass – Three conversion factors: molar Conversions • Problem Type 4 – Mass to mass – Three conversion factors: molar](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-16.jpg)
![Conversions • Tin(II) fluoride, Sn. F 2, is used in some toothpastes. It is Conversions • Tin(II) fluoride, Sn. F 2, is used in some toothpastes. It is](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-17.jpg)
![Conversions • Sodium peroxide reacts vigorously with water to produce sodium hydroxide and oxygen. Conversions • Sodium peroxide reacts vigorously with water to produce sodium hydroxide and oxygen.](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-18.jpg)
![Limiting Reactants • One reactant is present in excess • When one reactant is Limiting Reactants • One reactant is present in excess • When one reactant is](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-19.jpg)
![Limiting Reactants • C(s) + O 2(g) CO 2(g) – 5 mol C – Limiting Reactants • C(s) + O 2(g) CO 2(g) – 5 mol C –](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-20.jpg)
![Problem • Silicon dioxide (quartz) is usually quite unreactive but reacts readily with hydrogen Problem • Silicon dioxide (quartz) is usually quite unreactive but reacts readily with hydrogen](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-21.jpg)
![Problem • The black oxide of iron, Fe 3 O 4, occurs in nature Problem • The black oxide of iron, Fe 3 O 4, occurs in nature](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-22.jpg)
![Problem 3 Fe + 4 H 2 O Fe 3 O 4 + 4 Problem 3 Fe + 4 H 2 O Fe 3 O 4 + 4](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-23.jpg)
![Percent Yield • Theoretical yield – Maximum amount of product • Actual yield – Percent Yield • Theoretical yield – Maximum amount of product • Actual yield –](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-24.jpg)
![Problem • Chlorobenzene, C 6 H 5 Cl, is used in the production of Problem • Chlorobenzene, C 6 H 5 Cl, is used in the production of](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-25.jpg)
![C 6 H 6 + Cl 2 C 6 H 5 Cl + HCl C 6 H 6 + Cl 2 C 6 H 5 Cl + HCl](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-26.jpg)
![Problem • Huge quantities of sulfur dioxide are produced from zinc sulfide by means Problem • Huge quantities of sulfur dioxide are produced from zinc sulfide by means](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-27.jpg)
![Chapter Review • Pg. 295 – 8, 10, 11, 12, 14, 15, 22, 23, Chapter Review • Pg. 295 – 8, 10, 11, 12, 14, 15, 22, 23,](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-28.jpg)
- Slides: 28
![Chapter 9 Stoichiometry Chapter 9 Stoichiometry](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-1.jpg)
Chapter 9 Stoichiometry
![Stoichiometry Composition stoichiometry Mass relationships of elements in compounds Reaction stoichiometry Stoichiometry • Composition stoichiometry – Mass relationships of elements in compounds • Reaction stoichiometry](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-2.jpg)
Stoichiometry • Composition stoichiometry – Mass relationships of elements in compounds • Reaction stoichiometry – Mass relationships between reactants and products
![Reaction Stoichiometry Use ratios from balanced equation Problem Type 1 Given Reaction Stoichiometry • Use ratios from balanced equation • Problem Type 1 – Given](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-3.jpg)
Reaction Stoichiometry • Use ratios from balanced equation • Problem Type 1 – Given & unknown quantities in moles • Problem Type 2 – Given in moles & unknown in grams
![Reaction Stoichiometry Problem Type 3 Given in grams unknown in moles Reaction Stoichiometry • Problem Type 3 – Given in grams & unknown in moles](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-4.jpg)
Reaction Stoichiometry • Problem Type 3 – Given in grams & unknown in moles • Problem Type 4 – Given in grams & unknown in grams
![Mole Ratio Conversion factor that relates amount of moles of substances 2 Al Mole Ratio • Conversion factor that relates amount of moles of substances 2 Al](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-5.jpg)
Mole Ratio • Conversion factor that relates amount of moles of substances 2 Al 2 O 3(l) 4 Al(s) + 3 O 2(g) • How many moles of aluminum can be produced from 13. 0 mol of aluminum oxide?
![Molar Mass The mass in g of 1 mole of substance 2 Al Molar Mass • The mass (in g) of 1 mole of substance 2 Al](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-6.jpg)
Molar Mass • The mass (in g) of 1 mole of substance 2 Al 2 O 3(l) 4 Al(s) + 3 O 2(g) • How many grams of Al is equivalent to 26. 0 mol Al?
![Conversions Problem Type 1 Mole to mole One conversion factor mole Conversions • Problem Type 1 – Mole to mole – One conversion factor: mole](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-7.jpg)
Conversions • Problem Type 1 – Mole to mole – One conversion factor: mole ratio • Given (mol) x mole ratio (mol/mol) = unknown (mol)
![Conversions In a spacecraft the CO 2 exhaled by astronauts can be removed Conversions • In a spacecraft, the CO 2 exhaled by astronauts can be removed](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-8.jpg)
Conversions • In a spacecraft, the CO 2 exhaled by astronauts can be removed by its reaction with lithium hydroxide, Li. OH, according to the following chemical equation. CO 2(g) + 2 Li. OH(s) Li 2 CO 3(s) + H 2 O(l) • How many moles of Li. OH are required to react with 20 mol of CO 2, the average amount exhaled by a person each day?
![Conversions The disinfectant hydrogen peroxide H 2 O 2 decomposes to form water Conversions • The disinfectant hydrogen peroxide, H 2 O 2, decomposes to form water](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-9.jpg)
Conversions • The disinfectant hydrogen peroxide, H 2 O 2, decomposes to form water and oxygen gas. How many moles of O 2, will result from the decomposition of 5 mol of hydrogen peroxide?
![Conversions Problem Type 2 Mole to mass Two conversion factors mole Conversions • Problem Type 2 – Mole to mass – Two conversion factors: mole](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-10.jpg)
Conversions • Problem Type 2 – Mole to mass – Two conversion factors: mole ratio & molar mass • Given (mol) x mole ratio (mol/mol) x molar mass (g/mol) = unknown (g)
![Conversions In photosynthesis plants use energy from the sun to produce glucose C Conversions • In photosynthesis, plants use energy from the sun to produce glucose C](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-11.jpg)
Conversions • In photosynthesis, plants use energy from the sun to produce glucose C 6 H 12 O 6, and oxygen from the reaction of CO 2 and H 2 O. What mass, in grams, of glucose is produced when 3. 00 mol of H 2 O with CO 2?
![Conversions What mass of CO 2 in grams is needed to react with Conversions • What mass of CO 2, in grams, is needed to react with](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-12.jpg)
Conversions • What mass of CO 2, in grams, is needed to react with 3. 00 mol of H 2 O in the photosynthetic reaction described on the last slide?
![Conversions Problem Type 3 Mass to moles Two conversion factors molar Conversions • Problem Type 3 – Mass to moles – Two conversion factors: molar](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-13.jpg)
Conversions • Problem Type 3 – Mass to moles – Two conversion factors: molar mass & mole ratio • Given (g) x molar mass (mol/g) x mole ratio (mol/mol) = unknown (mol)
![Conversions The first step in the industrial manufacture of nitric acid is the Conversions • The first step in the industrial manufacture of nitric acid is the](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-14.jpg)
Conversions • The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia, NH 3(g) + O 2(g) NO(g) + H 2 O(g) (unbalanced) The reaction is run using 824 g of NH 3 and excess oxygen. a. How many moles of NO are formed? b. How many moles of H 2 O are formed?
![Conversions The compound Pt Cl 2NH 32 is effective as a treatment for Conversions • The compound Pt. Cl 2(NH 3)2 is effective as a treatment for](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-15.jpg)
Conversions • The compound Pt. Cl 2(NH 3)2 is effective as a treatment for some cancers. It is synthesized by the reaction shown in the following equation: K 2 Pt. Cl 4 + 2 NH 3 2 KCl + Pt. Cl 2(NH 3)2 a. How many moles of K 2 Pt. Cl 4 must react in order to produce 30. 0 g of Pt. Cl 2(NH 3)2? b. How many moles of NH 3 are needed to produce 30. 0 g of Pt. Cl 2(NH 3)2?
![Conversions Problem Type 4 Mass to mass Three conversion factors molar Conversions • Problem Type 4 – Mass to mass – Three conversion factors: molar](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-16.jpg)
Conversions • Problem Type 4 – Mass to mass – Three conversion factors: molar mass, mole ratio, molar mass • Given (g) x molar mass (mol/g) x mole ratio (mol/mol) x molar mass (g/mol) = unknown (g)
![Conversions TinII fluoride Sn F 2 is used in some toothpastes It is Conversions • Tin(II) fluoride, Sn. F 2, is used in some toothpastes. It is](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-17.jpg)
Conversions • Tin(II) fluoride, Sn. F 2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation. Sn + 2 HF Sn. F 2 + H 2 How many grams of Sn. F 2 are produced from the reaction of 30. 00 g of HF with Sn?
![Conversions Sodium peroxide reacts vigorously with water to produce sodium hydroxide and oxygen Conversions • Sodium peroxide reacts vigorously with water to produce sodium hydroxide and oxygen.](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-18.jpg)
Conversions • Sodium peroxide reacts vigorously with water to produce sodium hydroxide and oxygen. The unbalanced equation is the following: Na 2 O 2 + H 2 O Na. OH + O 2 a. What mass in grams of O 2 is produced when 50. 0 g of Na 2 O 2 react? b. What mass in grams of water is needed to react completely with the Na 2 O 2?
![Limiting Reactants One reactant is present in excess When one reactant is Limiting Reactants • One reactant is present in excess • When one reactant is](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-19.jpg)
Limiting Reactants • One reactant is present in excess • When one reactant is used up reaction is over • Limiting reactant – Limits the production of product • Excess reactant – Not completely used up
![Limiting Reactants Cs O 2g CO 2g 5 mol C Limiting Reactants • C(s) + O 2(g) CO 2(g) – 5 mol C –](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-20.jpg)
Limiting Reactants • C(s) + O 2(g) CO 2(g) – 5 mol C – 10 mol O 2 – More than enough O 2 - 5 mol excess – Limiting - Carbon
![Problem Silicon dioxide quartz is usually quite unreactive but reacts readily with hydrogen Problem • Silicon dioxide (quartz) is usually quite unreactive but reacts readily with hydrogen](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-21.jpg)
Problem • Silicon dioxide (quartz) is usually quite unreactive but reacts readily with hydrogen fluoride according to the following equation. Si. O 2 + 4 HF Si. F 4 + 2 H 2 O If 2. 0 mol of HF are exposed to 4. 5 mol of Si. O 2, which is the limiting reactant?
![Problem The black oxide of iron Fe 3 O 4 occurs in nature Problem • The black oxide of iron, Fe 3 O 4, occurs in nature](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-22.jpg)
Problem • The black oxide of iron, Fe 3 O 4, occurs in nature as the mineral magnetite. This substance can also be made in the laboratory by the reaction between redhot iron and steam according to the following equation. 3 Fe + 4 H 2 O Fe 3 O 4 + 4 H 2
![Problem 3 Fe 4 H 2 O Fe 3 O 4 4 Problem 3 Fe + 4 H 2 O Fe 3 O 4 + 4](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-23.jpg)
Problem 3 Fe + 4 H 2 O Fe 3 O 4 + 4 H 2 a. When 36. 0 g of H 2 O is mixed with 167 g of Fe, which is the limiting reactant? b. What mass in grams of black iron oxide is produced? c. What mass in grams of excess reactant remains when the reaction is completed?
![Percent Yield Theoretical yield Maximum amount of product Actual yield Percent Yield • Theoretical yield – Maximum amount of product • Actual yield –](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-24.jpg)
Percent Yield • Theoretical yield – Maximum amount of product • Actual yield – Measured amount of product produced • Efficiency express in percent yield % yield = (actual yield)/(theoretical yield) x 100
![Problem Chlorobenzene C 6 H 5 Cl is used in the production of Problem • Chlorobenzene, C 6 H 5 Cl, is used in the production of](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-25.jpg)
Problem • Chlorobenzene, C 6 H 5 Cl, is used in the production of many important chemicals, such as aspirin, and disinfectants. One industrial method of preparing chlorobenzene is to react benzene, C 6 H 6, with chlorine, which is represented by the following equation.
![C 6 H 6 Cl 2 C 6 H 5 Cl HCl C 6 H 6 + Cl 2 C 6 H 5 Cl + HCl](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-26.jpg)
C 6 H 6 + Cl 2 C 6 H 5 Cl + HCl • When 36. 8 g of C 6 H 6 react with an excess of Cl 2, the actual yield of C 6 H 5 Cl is 38. 8 g. What is the percent yield of C 6 H 5 Cl?
![Problem Huge quantities of sulfur dioxide are produced from zinc sulfide by means Problem • Huge quantities of sulfur dioxide are produced from zinc sulfide by means](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-27.jpg)
Problem • Huge quantities of sulfur dioxide are produced from zinc sulfide by means of the following reaction. 2 Zn. S + 3 O 2 2 Zn. O + 2 SO 2 If the typical yield is 86. 78%, how much SO 2 should be expected if 4897 g of Zn. S are used
![Chapter Review Pg 295 8 10 11 12 14 15 22 23 Chapter Review • Pg. 295 – 8, 10, 11, 12, 14, 15, 22, 23,](https://slidetodoc.com/presentation_image/3fbaa0cee060c6ae4711725080d09442/image-28.jpg)
Chapter Review • Pg. 295 – 8, 10, 11, 12, 14, 15, 22, 23, 24, 26, 28, 33
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