ii. stoichiometry in the real world (p. 379 – 388) stoichiometry – ch. 11
TRANSCRIPT
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II. Stoichiometry in the Real World
(p. 379 – 388)
Stoichiometry – Ch. Stoichiometry – Ch. 1111
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
Available IngredientsAvailable Ingredients• 4 slices of bread• 1 jar of peanut butter• 1/2 jar of jelly
Limiting ReactantLimiting Reactant• bread
Excess ReactantsExcess Reactants• peanut butter and jelly
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
Available IngredientsAvailable Ingredients• 24 graham cracker squares• 1 bag of marshmallows• 12 pieces of chocolate
Limiting ReactantLimiting Reactant• chocolate
Excess ReactantsExcess Reactants• Marshmallows and graham
crackers
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
Limiting ReactantLimiting Reactant• one that is used up in a reaction• determines the amount of product that
can be produced
Excess ReactantExcess Reactant• added to ensure that the other reactant
is completely used up• cheaper & easier to recycle
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
1. Write the balanced equation.
2. For each reactant, calculate the
amount of product formed.
3. Smaller answer indicates:
• limiting reactant
• amount of product actually possible
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
79.1 g of zinc react with 68.1 g HCl. Identify the limiting and excess reactants. How many grams of hydrogen can be formed?
Zn + 2HCl ZnCl2 + H2 79.1 g ? g68.1 g
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
79.1g Zn
1 molZn
65.39g Zn
= 2.44 g H2
1 molH2
1 molZn
2.02 gH2
1 molH2
Zn + 2HCl ZnCl2 + H2 79.1 g ? g68.1 g
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
2.02 g H2
1 molH2
68.1g HCl
1 molHCl
36.46 g HCl
= 1.89 g H2
1 molH2
2 molHCl
Zn + 2HCl ZnCl2 + H2 79.1 g ? g68.1 g
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
Zn: 2.44 g H2 HCl: 1.89 g H2
Limiting reactant: HCl
Excess reactant: Zn
Product Formed: 1.89 g H2
left over zinc
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A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2
5.42 g of magnesium ribbon react with 4.00 g of oxygen gas. Identify the limiting and excess reactants. How many grams of magnesium oxide are formed?
2Mg + O2 2MgO 5.42 g ? g4.00 g
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A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2
5.42g Mg
1 molMg
24.31g Mg
= 8.99 g MgO
2 molMgO
2 molMg
40.31 gMgO
1 molMgO
2Mg + O2 2MgO
5.42 g ? g4.00 g
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A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2
40.31g MgO
1 molMgO
4.00g O2
1 molO2
32.00 g O2
= 10.1 g MgO
2 molMgO
1 molO2
2Mg + O2 2MgO
5.42 g ? g4.00 g
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A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2A. Limiting Reactants #2
Mg: 8.99 g MgO O2: 10.1 g MgO
Excess oxygen
Limiting reactant: Mg
Excess reactant: O2
Product Formed: 8.99 g MgO
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A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants
What other information could you find in these problems?
• How much of each reactant is used – in grams, liters, moles
• How much of excess reactant is left over – in grams, liters, moles
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B. Percent YieldB. Percent YieldB. Percent YieldB. Percent Yield
100yield ltheoretica
yield actualyield %
calculated on paper
measured in lab
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B. Percent YieldB. Percent YieldB. Percent YieldB. Percent Yield
When 45.8 g of K2CO3 react with excess
HCl, 46.3 g of KCl are formed. Calculate the theoretical and % yields of KCl.