Presentation is loading. Please wait.

Presentation is loading. Please wait.

4. Balancing Reactions How are coefficients different from subscripts? 2H 2 + O 2  2H 2 O subscripts = # of atoms.

Similar presentations


Presentation on theme: "4. Balancing Reactions How are coefficients different from subscripts? 2H 2 + O 2  2H 2 O subscripts = # of atoms."— Presentation transcript:

1 4. Balancing Reactions How are coefficients different from subscripts? 2H 2 + O 2  2H 2 O subscripts = # of atoms

2 4. Balancing Reactions How are coefficients different from subscripts? 2H 2 + O 2  2H 2 O coefficients = how many

3 4. Balancing Reactions 2H 2 + O 2  2H 2 O subscripts = # of atoms coefficients = how many

4 4. Balancing Reactions H 2 + O 2  H 2 O 2 subscripts = # of atoms coefficients = how many

5 New Unit: Stoichiometry OBJECTIVE: Balancing Reactions + Grams  Moles + Moles  Grams

6 Topics to be Covered 1. What is Stoichiometry? 2. 1 Step Conversions 3. 2 Step Conversions 4. 3 Step Conversions 5. Limiting Reactants 6. Percentage Yield

7 What is Stoichiometry? ▪ It is: – The QUANTITATIVE relationships between reactants and products – Using MATH and NUMBERS to calculate reactants and products 1. What is Stoichiometry?

8 1. What is Stoichiometry Balanced Reactions are like recipes

9 1. What is Stoichiometry What information is missing?? butter brown sugar egg flour baking soda salt + chocolate chips cookies

10 1. What is Stoichiometry What information Is missing?? 3/4 butter 1/2 brown sugar 1 egg 1 1/2 flour 1 baking soda 1/4 salt + 1 chocolate chips 30 cookies

11 1. What is Stoichiometry Balanced Reactions are like recipes 3/4 cup butter 1/2 cup brown sugar 1 egg 1 1/2 cups flour 1 teaspoon baking soda 1/4 teaspoon salt + 1 cup chocolate chips 30 cookies

12

13 Fundamental Measurements What we measure UNIT ▪ Distance ▪ Mass ▪ Time ▪ Electric current ▪ Temperature ▪ Amount ▪ Intensity of light ▪ Meter ▪ Gram ▪ Seconds ▪ Amps ▪ Kelvin ▪ Mole ▪ Candela

14 Fundamental Measurements What we measure UNIT ▪ Distance ▪ Mass ▪ Time ▪ Electric current ▪ Temperature ▪ Amount ▪ Intensity of light ▪ Meter ▪ Gram ▪ Seconds ▪ Amps ▪ Kelvin ▪ Mole ▪ Candela

15 1. What is Stoichiometry? KI + Pb(NO 3 ) 2  PbI 2 + KNO 3

16 1. What is Stoichiometry? 2KI + Pb(NO 3 ) 2  PbI 2 + 2KNO 3 COEFFICIENTS = amount of MOLES KI = 2 moles Pb(NO 3 ) 2 = 1 mole PbI 2 = 1 mole KNO 3 = 2 moles

17 1. What is Stoichiometry? 2KI + Pb(NO 3 ) 2  PbI 2 + 2KNO 3 Stoichiometry = using coefficients from balanced reactions to convert grams  moles and much more.

18 2. 1 Step Conversions OBJECTIVE: Use stoichiometry to solve calculation problems

19 2. 1 Step Conversions 2H 2 + O 2  2H 2 O You have 3 moles of O 2 How many moles of H 2 O can you produce? How do you solve something like this?

20 2. 1 Step Conversions 2H 2 + O 2  2H 2 O How do you solve something like this? 1.Balance Reaction first!!! 2.Sideways T and MOLE RATIO

21 1. 2Na + Cl 2  2NaCl 5 moles of Na = ? moles NaCl? 2. CH 4 + 2O 2  CO 2 + 2H 2 O 2 moles of CH 4 = ? moles CO 2 ? 3. Cu + 2AgNO 3  2Ag + Cu(NO 3 ) 2 4 moles of AgNO 3 = ? moles Ag? 4. 2KI + Pb(NO 3 ) 2  PbI 2 + 2KNO 3 43 moles of KI = ? moles KNO 3 ? 2. 1 Step Conversions

22 3.2-Step Conversions OBJECTIVE: Grams  Moles  Mole Ratio

23 3. 2-Step Conversions 2H 2 + O 2  2H 2 O You have 64 grams of O 2 How many moles of H 2 O can you produce? How do you solve something like this?

24 3. 2-Step Conversions 2H 2 + O 2  2H 2 O You have 64 grams of O 2 How many moles of H 2 O can you produce? How do you solve something like this? 1. Balance2. Grams -> Moles3. Mole Ratio

25

26

27 4. 3-Step Conversions & Alternate Routes OBJECTIVE: Add more routes to Stoichiometry Highway

28 4. 3-Step Conversions

29 Avogadro Avenue 2H 2 + O 2  2H 2 O 12.04 x 10 23 particles of H 2 How many moles of H 2 O?

30 4. 3-Step Conversions

31 Liter Lane 2H 2 + O 2  2H 2 O 44.8 L of H 2 How many moles of H 2 O?

32 4. 3 Step Conversions and Alternate Routes 1.C 5 H 12  C 5 H 8 + 2H 2 1.89 x 10 24 molecules of C 5 H 12. How many molecules of C 5 H 8 ? 2.Br 2 + 5F 2  2BrF 5 2.89 x 10 24 molecules of Br 2. How many molecules of BrF 5 ? 1.11 x 10 20 molecules of F 2. How many molecules of BrF 5 ? 3.C 5 H 12  C 5 H 8 + 2H 2 1.366 L of C 5 H 12. How many liters of C 5 H 8 ? 2.0.0973 L of C 5 H 12. How many liters of C 5 H 8 ? 3.1.98 L of C 5 H 12. How many liters of H 2 ?

33 1. C 5 H 12  C 5 H 8 + 2H 2 1.89 x 10 24 molecules of C 5 H 12. How many molecules of C 5 H 8 ? 2. Br 2 + 5F 2  2BrF 5 2.89 x 10 24 molecules of Br 2. How many molecules of BrF 5 ? 1.11 x 10 20 molecules of F 2. How many molecules of BrF 5 ? 3. C 5 H 12  C 5 H 8 + 2H 2 1. 366 L of C 5 H 12. How many liters of C 5 H 8 ? 2. 0.0973 L of C 5 H 12. How many liters of C 5 H 8 ? 3. 1.98 L of C 5 H 12. How many liters of H 2 ?

34 4. 3 Step Conversions and Alternate Routes 1.C 5 H 12  C 5 H 8 + 2H 2 1.89 x 10 24 molecules of C 5 H 12. How many molecules of C 5 H 8 ? 2.Br 2 + 5F  2BrF 5 2.89 x 10 24 molecules of Br 2. How many molecules of BrF 5 ? 1.11 x 10 20 molecules of F 2. How many molecules of BrF 5 ?

35 5. Limiting Reactants OBJECTIVE: Running out of “ingredients”

36 5. Limiting Reactants 8 buns + 12 patties Which will run out first?

37 Limiting Reactant Excess Reactant ▪ The reactant that controls the quantity of product that can form in a chemical reaction ▪ Stuff that runs out first ▪ The reactant that is not completely used up in a chemical reaction ▪ Stuff left over

38 5. Limiting Reactants 8 buns + 12 patties Which is limiting?

39 5. Limiting Reactants 4 franks + 12 buns Which is limiting?

40 2 H 2 + O 2  2 H 2 O – 10 moles of H2 – 10 moles of O2. – How many moles of H 2 O? How to Solve? Identify limiting reactant. Limiting Reactant = Smaller Number 5. Limiting Reactants

41 Fe + S  Fe 2 S 3 2 Fe + 3 S  Fe 2 S 3 – 12 moles of Fe – 12 moles of S – How many moles of Fe 2 S 3 ? (Identify limiting reactant) WHAT IS FIRST STEP? BALANCE 5. Limiting Reactants

42 NO +Cl 2  NOCl – 4 mol of NO – 4 mol of Cl 2 – How many mol of NOCl? BALANCE FIRST!! 5. Limiting Reactants

43 NO +Cl 2  NOCl – 100g of NO – 100g of Cl 2 – How many mol of NOCl? 5. Limiting Reactants

44 Fe + S  Fe 2 S 3 – 10 moles of Fe – 12 moles of S. – How many moles of Fe 2 S 3 ? Identify limiting reactant. – 150 g of Fe – 120g of S. – How many grams of Fe 2 S 3 ? ▪ Go to Word Document 5. Limiting Reactants

45 H 2 +N 2  NH 3 – 12L of H 2 – 10L of N 2 – How many grams of NH 3 ? – 25g of H 2, 35g of N 2. How many liters of NH 3 ? 5. Limiting Reactants

46 6. Percentage Yield OBJECTIVE: Measuring Efficiency

47

48

49

50

51 6. Percentage Yield Efficiency of a reaction = Percentage Yield

52 Formula for Percentage Yield 6. Percentage Yield

53 Actual Yield Theoretical Yield ▪ What is actually produced. ▪ What you have been calculating so far ▪ If reaction occurs with 100% efficiency

54 2Al + 6HCl -> 2AlCl 3 + 3H 2 You calculated a theoretical yield of 8.77 grams for AlCl 3. But only 5.66 grams of AlCl 3 is actually produced. What is the percentage yield? You calculated a theoretical yield of 9.79 grams for H 2. The actual yield for H 2 is 4.04. What is the percentage yield?

55 6. Percentage Yield 2Al + 6HCl -> 2AlCl 3 + 3H 2 The theoretical yield is 98.5 grams for AlCl3. This reaction has 77 percentage yield. What is the actual yield?

56 2H 2 O 2 -> 2H 2 O +O 2 1.How many L of O 2 is produced from 250g of H 2 O 2 ? 2.If reaction has 68% yield, how many L of O 2 is actually produced?

57 2P +Cl 2 -> 2PCL 3 1.500L (actual yield) of PCl3 needs to be produced. 2.The reaction as a 75% yield. How many grams of Cl2 is needed?

58 2P +Cl 2 -> 2PCL 3 1.450g of P, 448L Cl 2, ?g of PCl 3 2.Actual Yield is 148g, what is % yield? 3.If % Yield is 48%, how much PCl 3 would actually be produced 4.Suppose P is in excess, and 300g of PCl 3 needed to be produced. The % Yield is 72%. How many L of Cl 2 is needed?

59 3H 2 + N 2 -> 2NH 3 1.40L of H 2, 15L of N 2, ?g of NH 3 2.Actual Yield is 17.9L of NH 3, what is % Yield? 3.If reaction has % Yield of 82%, how many molecules of NH 3 would be produced? 4.N2 is in excess, reaction has 62% Yield. 500L of NH 3 need to produced. How many g of H 2 is needed?


Download ppt "4. Balancing Reactions How are coefficients different from subscripts? 2H 2 + O 2  2H 2 O subscripts = # of atoms."

Similar presentations


Ads by Google