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Chapter 4: Balancing Equations and Stoichiometry.

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Presentation on theme: "Chapter 4: Balancing Equations and Stoichiometry."— Presentation transcript:

1 Chapter 4: Balancing Equations and Stoichiometry

2 Key Terms & Concepts  Stoichiometry  Chemical Equations  reactants and products  balancing chemical equations  Chemical Calculations  Limiting Reactant  Theoretical and Percent Yield

3 Stoichiometry  Stoichiometry is the study of the quantitative nature of chemical formulas and chemical reactions.  Stoichiometry is one the the most essential tools in chemistry  It allows to quantify everything from global warming to drug manufacturing

4 Chemical Equations  Chemical reactions are represented in a concise manner by chemical equation  For example, when H 2 burns in O 2, H 2 O is formed.  The chemical equation for this reaction is: 2 H 2 + O 2  2H 2 O

5 Chemical Equations 2 H 2 + O 2  2 H 2 O  The compounds on the left of the arrow are called “reactants”  The compounds on the right of the arrow are called “products”  H 2 and O 2 are reactants, H 2 O is the product

6 Chemical Equations 2 H 2 + O 2  2 H 2 O  Notice that the number of atoms or each element is equal on both sides of the equation  4 H, 2 0  All chemical equations must meet this requirement  Chemical equations must be balanced!!  We balance equations by changing coefficients, not chemical formulas

7 Chemical Equations

8  Consider the following chemical equation CH 4 + O 2  CO 2 + H 2 O unbalanced  Start with elements that only appear in one compound on either side of the equation  C and H are only in one compound on either side  C is balanced

9 Chemical Equations CH 4 + O 2  CO 2 + H 2 O unbalanced  4 H’s in reactants, 2 H’s in products  Put coefficient of 2 in front of H 2 O  4 H’s in reactants, 4 H’s in products CH 4 + O 2  CO H 2 O unbalanced

10 Chemical Equations CH 4 + O 2  CO H 2 O unbalanced  2 O’s in reactants, 4 O’s in products  Put coefficient of 2 in front of O 2  4 O’s in reactants, 4 O’s in products CH O 2  CO H 2 O balanced

11 Chemical Equations

12  Consider this equation: C 3 H 8 + O 2  CO 2 + H 2 O 3C + 8H + 2O  1C + 2H + 3O

13 Chemical Equations  Balance C and H C 3 H 8 + O 2  3CO 2 + 4H 2 O 3C + 8H + 2O  3C + 8H + 10O

14 Chemical Equations  Balance O C 3 H 8 + 5O 2  3CO 2 + 4H 2 O 3C + 8H + 10O  3C + 8H + 10O

15 Chemical Equations  Example 4.1 Balance the following chemical equations (1) Mg + HCl  MgCl 2 + H 2 (2) K + H 2 O  KOH + H 2 (3) CaCl 2 + Na 3 PO 4  Ca 3 (PO 4 ) 2 + NaCl (4) NaN 3  Na + N 2 (5) C 8 H 18 + O 2  CO 2 + H 2 O

16 Chemical Equations  Example 4.1 Balance the following chemical equations (1) Mg + 2 HCl  MgCl 2 + H 2 (2) 2 K + 2 H 2 O  2 KOH + H 2 (3) 3 CaCl Na 3 PO 4  Ca 3 (PO 4 ) NaCl (4) 2 NaN 3  2 Na + 3 N 2 (5) 2 C 8 H O 2  16 CO H 2 O

17 Chemical Equations  Example 4.2 Write a balanced chemical equation for the following reactions (1)ammonium nitrate decomposes to nitrogen gas, oxygen gas, and water (2)iron reacts with oxygen gas and water to form iron(II) hydroxide (3)ammonia reacts with oxygen gas to produce nitrogen monoxide and water

18 Chemical Equations  Example 4.2 Write a balanced chemical equation for the following reactions (1) 2 NH 4 NO 3  2 N 2 + O H 2 O (2) 2 Fe + O H 2 O  2 Fe(OH) 2 (3) 4NH O 2  4 NO + 6 H 2 O

19 Chemical Calculations 2 H 2 + O 2  2 H 2 O 2 molecules 1 molecule2 molecules 2(6.022x10 23 ) molecules 6.022x10 23 molecules 2(6.022x10 23 ) molecules 2 mol 1 mol2 mol  Stoichiometric coefficients can be interpreted as either number of molecules or number of moles.

20 Chemical Calculations  Example 4.3 How many moles of water can be produced from 5.25 mol O 2 ?

21 Chemical Calculations  Example 4.4 How many moles of oxygen are required to completely react with 8.50 moles of butane, C 4 H 10 ?

22 Chemical Calculations  We can’t directly measure moles. We can measure mass.  We can use the stoichiometric coefficients of a reaction to determine the mass relationships.  However, we must always convert mass to moles.  We cannot directly compare the masses of reactants and products.  We can only compare the moles of reactants and products.

23 Chemical Calculations  The general scheme is:

24 Chemical Calculations  Example 4.5 Geranyl formate is used as a synthetic rose essence in cosmetics. The compound is prepared from formic acid and geraniol: HCOOH + C 10 H 18 O  C 11 H 18 O 2 + H 2 O A chemist needs to make some geranyl formate for a batch of perfume. How many grams of geranyl formate can a chemist make from 375g of geraniol?

25 Chemical Calculations

26  Example 4.6 Solid lithium hydroxide is used in space vehicles to remove exhaled carbon dioxide. The lithium hydroxide reacts with gaseous carbon dioxide to form solid lithium carbonate and liquid water. How many grams of carbon dioxide can be absorbed by each 1.00 g of lithium hydroxide? 2 LiOH (s) + CO 2 (g)  Li 2 CO 3 (g) + H 2 O (l)

27 Chemical Calculations  Example LiOH (s) + CO 2 (g)  Li 2 CO 3 (g) + H 2 O (l)

28 Theoretical and Percent Yield  The amount of product that can be produced from a given amount of reactants is the theoretical yield.  However, no reaction goes to actual completion. The amount of products that is actually produced from a given amount of reactants is the actual yield. Some reactants may not react Reactants may react in an undesired way (side reactions) May be difficult to remove products from pot

29 Theoretical and Percent Yield  The extent of the desired reaction is typically reported as the percent yield.

30 Theoretical and Percent Yield  Example 4.7 Look back at Example 4.5. If the chemist starts with 375g of geraniol and collects 417g of purified product, what is the percent yield of the synthesis?

31 Theoretical and Percent Yield  Example g of sodium metal is burned in an excess of chlorine gas. What is the theoretical yield of sodium chloride? If 54.8 g of sodium chloride is actually produced, what is the percent yield of the reaction? 2 Na + Cl 2  2 NaCl

32 Theoretical and Percent Yield

33

34  Example 4.9 Titanium is a strong, lightweight, corrosion- resistant metal that is used in aeronautics and bicycle frames. It is prepared by the reaction of titanium (IV) chloride with molten magnesium between 950  C and 1150  C. TiCl 4 (g) + 2 Mg(l)  Ti(s) + 2 MgCl 2 (l) In a certain industrial process 3.54x10 7 g of TiCl 4 are reacted with 1.13x10 7 g of Mg. (a)Calculate the theoretical yield of Ti in grams. (b)Calculate the percent yield if 7.91x10 6 g of Ti are actually produced.

35 Theoretical and Percent Yield

36

37 Limiting Reactants  Most reactions do not occur with stoichiometric equivalent amounts of each reactant. One reactant is used up first This reactant is the limiting reactant because it limits the amount of products that can be formed

38 Limiting Reactants  Consider the “ham sandwich” example one sandwich is made from one slice of ham, one slice of cheese and two slices of bread How many ham sandwiches can be made from six slices of ham, seven slices of cheese and 14 slices of bread? What is the limiting reactant?

39 Limiting Reactants

40  If a problem gives specific amounts of two or more reactants it is a limiting reactant problem.  Determine the amount of product that can be formed from each reactant The reactant which produces the smallest amount of product is the limiting reactant The remaining reactants are said to be in excess

41 Limiting Reactants  Example 4.10 How many moles of water can be formed when 10.0 moles of H 2 reacts with 4.50 moles of O 2 ? What is the limiting reactant?

42 Limiting Reactants  Example H 2 + O 2  2 H 2 O

43 Limiting Reactants  Example 4.11 Solutions of sulfuric acid and lead (II) acetate react to form solid lead (II) sulfate and aqueous acetic acid. If 15.0 g of sulfuric acid and 15.0 g of lead (II) acetate are mixed, calculate the number of grams of lead (II) sulfate that can be produced. Also calculate the number of grams of the excess reagent remaining after the reaction is completed.

44 Limiting Reactants H 2 SO 4 + Pb(CH 3 COO) 2  PbSO CH 3 COOH

45 Limiting Reactants

46 End-of-Chapter Exercises  Suggested End-of-Chapter Exercises 5, 9, 10, 14, 17, 20, 22, 28


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