Limiting Reagents & Percent Yield Chapter 9 Notes Part III.
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Transcript of Limiting Reagents & Percent Yield Chapter 9 Notes Part III.
Limiting ReagentsLimiting Reagents& Percent Yield& Percent Yield
Chapter 9 Notes Part IIIChapter 9 Notes Part III
What are limiting reagents?
Up until now, we have assumed that all reactants are used up in a reaction.
In actuality, usually one chemical runs out first, stopping the reaction—that chemical is called the limiting reagent.
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
+
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
+
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
+ +
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
+ +
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
+ + =
For Example:
How many sandwiches can you make from a full jar of peanut butter, a full jar of jelly and 4 slices of bread?
+ + =
The The limiting reagentlimiting reagent limits or limits or determines the amount of product determines the amount of product that can be formed in a reaction.that can be formed in a reaction.
On the flip side, the On the flip side, the excess excess reagentreagent is the one not is the one not
completely used up.completely used up.
How do you find what the limiting reagent is?
To find the limiting reagent, use dimensional analysis to determine how much of the product will be formed by both reactants.
The smaller of the two results will indicate which reactant is the limiting reagent.
Here’s an example:Here’s an example:
In the reaction: In the reaction:
Mg + HCl Mg + HCl MgCl MgCl22 + H + H22
you combine 35.5 grams of you combine 35.5 grams of magnesium with 28.1 grams of magnesium with 28.1 grams of
hydrochloric acid. Which one is hydrochloric acid. Which one is the limiting reagent, and how the limiting reagent, and how much magnesium chloride is much magnesium chloride is
produced?produced?
Mg + Mg + 22 HCl HCl MgCl MgCl22 + H + H22
Mg + Mg + 22 HCl HCl MgCl MgCl22 + H + H22
35.5 g Mg x 35.5 g Mg x 1 mole Mg1 mole Mg x x 1 mole MgCl1 mole MgCl22 x x 95.3 g MgCl95.3 g MgCl22 = 139 g MgCl = 139 g MgCl22
24.3 g Mg 1 mole Mg 1 mole MgCl24.3 g Mg 1 mole Mg 1 mole MgCl22
Mg + Mg + 22 HCl HCl MgCl MgCl22 + H + H22
35.5 g Mg x 35.5 g Mg x 1 mole Mg1 mole Mg x x 1 mole MgCl1 mole MgCl22 x x 95.3 g MgCl95.3 g MgCl22 = 139 g MgCl = 139 g MgCl22
24.3 g Mg 1 mole Mg 1 mole MgCl24.3 g Mg 1 mole Mg 1 mole MgCl22
28.1 g HCl x 28.1 g HCl x 1 mole HCl1 mole HCl x x 1 mole MgCl1 mole MgCl22 x x 95.3 g MgCl95.3 g MgCl22 = 36.6 g MgCl = 36.6 g MgCl22
36.5 g HCl 2 moles HCl 1 mole MgCl36.5 g HCl 2 moles HCl 1 mole MgCl22
Mg + Mg + 22 HCl HCl MgCl MgCl22 + H + H22
35.5 g Mg x 35.5 g Mg x 1 mole Mg1 mole Mg x x 1 mole MgCl1 mole MgCl22 x x 95.3 g MgCl95.3 g MgCl22 = 139 g MgCl = 139 g MgCl22
24.3 g Mg 1 mole Mg 1 mole MgCl24.3 g Mg 1 mole Mg 1 mole MgCl22
28.1 g HCl x 28.1 g HCl x 1 mole HCl1 mole HCl x x 1 mole MgCl1 mole MgCl22 x x 95.3 g MgCl95.3 g MgCl22 = 36.6 g MgCl = 36.6 g MgCl22
36.5 g HCl 2 moles HCl 1 mole MgCl36.5 g HCl 2 moles HCl 1 mole MgCl22
HCl is the limiting reagent and HCl is the limiting reagent and
36.6 g of MgCl36.6 g of MgCl2 2 are produced.are produced.
Percent YieldIn the real world, you never form In the real world, you never form
100% of the products that you think 100% of the products that you think you should based on theoretical you should based on theoretical calculations.calculations.
By comparing how much of a product By comparing how much of a product forms to how much should form forms to how much should form based on stoichiometry, you can based on stoichiometry, you can find the percent yield.find the percent yield.
Percent Yield %Yield= actual yield x 100
theoretical yield
Practice ProblemIn the reaction of nitrogen gas In the reaction of nitrogen gas
and hydrogen gas producing and hydrogen gas producing ammonia (NHammonia (NH33), 250.2g H), 250.2g H22
produces 1095.1g NHproduces 1095.1g NH33. What . What
is the % yield of this reaction?is the % yield of this reaction?
N2 + 3 H2 → 2 NH3
First find out how much NH3 should be produced:
N2 + 3 H2 → 2 NH3
First find out how much NH3 should be produced:
250.2 g H2 x 1 mole H2 x 2 moles NH3 x 17 g NH3 = 2836 g NH3
1 g H2 3 moles H2 1 mole NH3
N2 + 3 H2 → 2 NH3
First find out how much NH3 should be produced:
250.2 g H2 x 1 mole H2 x 2 moles NH3 x 17 g NH3 = 2836 g NH3
1 g H2 3 moles H2 1 mole NH3
Then calculate the percent yield:
N2 + 3 H2 → 2 NH3
First find out how much NH3 should be produced:
250.2 g H2 x 1 mole H2 x 2 moles NH3 x 17 g NH3 = 2836 g NH3
1 g H2 3 moles H2 1 mole NH3
Then calculate the percent yield:% Yield = Actual x 100 % Yield = 1095.1 g x 100
Theor. 2836 g
% Yield = 38.6 %
N2 + 3 H2 → 2 NH3
First find out how much NH3 should be produced:
250.2 g H2 x 1 mole H2 x 2 moles NH3 x 17 g NH3 = 2836 g NH3
1 g H2 3 moles H2 1 mole NH3
Then calculate the percent yield:% Yield = Actual x 100 % Yield = 1095.1 g x 100
Theor. 2836 g
% Yield = 38.6 %
Reaction #1
KK22CrOCrO44 + Pb(NO + Pb(NO33))22 KNO KNO33 + PbCrO + PbCrO44
If 0.947g KIf 0.947g K22CrOCrO44 are combined are combined
with 0.331g Pb(NOwith 0.331g Pb(NO33))22 what what
will be the limiting reagent, will be the limiting reagent, and how much lead and how much lead chromate is produced?chromate is produced?
KK22CrOCrO44 + Pb(NO + Pb(NO33))22 2 KNO 2 KNO33 + PbCrO + PbCrO44
0.947g K2CrO4 x 1 mole K2CrO4 x 1 mole PbCrO4 x 323.2 g PbCrO4 = 1.97 g PbCrO4
155.1 g K2CrO4 1 mole K2CrO4 1 mole PbCrO4
0.331g Pb(NO0.331g Pb(NO33))22 x x 1 mole Pb(NO1 mole Pb(NO33))22 x x 1 mole PbCrO4 x 323.2 g PbCrO4 = 0.323 g PbCrO4
331.2 g Pb(NOPb(NO33))22 1 mole Pb(NO 1 mole Pb(NO33))2 2 1 mole PbCrO4
Pb(NOPb(NO33))22 is the limiting reagent and is the limiting reagent and
0.323 g PbCrO0.323 g PbCrO44 is produced. is produced.
Reaction #2
CC33HH88O + OO + O22 CO CO22 + H + H22OO
If 3.78 L of OIf 3.78 L of O22 are combined with are combined with
7.9 g of C7.9 g of C33HH88O, what is the O, what is the
limiting reagent, and how much limiting reagent, and how much water is produced?water is produced?
2 C2 C33HH88O + 9 OO + 9 O22 6 CO 6 CO22 + 8 H + 8 H22OO
3.78 L of O3.78 L of O2 2 x x 1 mole O1 mole O22 x x 8 moles H8 moles H22OO x x 18 g H18 g H22OO = 2.7 g H = 2.7 g H22OO
22.4 L O22.4 L O22 9 moles O 9 moles O22 1 mole H 1 mole H22OO
7.9 g of C7.9 g of C33HH88O x O x 1 mole C1 mole C33HH88OO x x 8 moles H8 moles H22OO x x 18 g H18 g H22OO = 9.48 g H = 9.48 g H22OO
60 g C60 g C33HH88O 2 moles CO 2 moles C33HH88O 1 mole HO 1 mole H22OO
OO22 is the limiting reagent and 2.7 g of H is the limiting reagent and 2.7 g of H22O are produced.O are produced.
Reaction #3
KK22CrOCrO44 + AgNO + AgNO33 KNO KNO33 + Ag + Ag22CrOCrO44
If 1.17g KIf 1.17g K22CrOCrO44 are combined with are combined with
1.23g AgNO1.23g AgNO33, what is the limiting , what is the limiting
reagent and how much Agreagent and how much Ag22CrOCrO44 is is
produced?produced?
KK22CrOCrO44 + 2 AgNO + 2 AgNO33 2 KNO 2 KNO33 + Ag + Ag22CrOCrO44
1.17g K1.17g K22CrOCrO44 x x 1 mole K1 mole K22CrOCrO44 x x 1 mole Ag1 mole Ag22CrOCrO44 x x 331.8 g Ag331.8 g Ag22CrOCrO44 = 1.99 g Ag = 1.99 g Ag22CrOCrO44
194.2 g K194.2 g K22CrOCrO44 1 mole K 1 mole K22CrOCrO44 1 mole Ag 1 mole Ag22CrOCrO44
1.23g AgNO1.23g AgNO3 3 x x 1 mole AgNO1 mole AgNO33 x x 1 mole Ag1 mole Ag22CrOCrO44 x x 331.8 g Ag331.8 g Ag22CrOCrO44 = 1.20 g Ag = 1.20 g Ag22CrOCrO44
169.9 g AgNO169.9 g AgNO33 2 moles AgNO 2 moles AgNO33 1 mole Ag 1 mole Ag22CrOCrO44
AgNOAgNO33 is the limiting reagent and is the limiting reagent and
1.20 g Ag1.20 g Ag22CrOCrO44 are produced. are produced.
Reaction #4
Zn + HCl Zn + HCl ZnCl ZnCl22 + H + H22
What is the limiting reagent and What is the limiting reagent and how many liters of hydrogen how many liters of hydrogen are produced if 15.5 grams of are produced if 15.5 grams of zinc are combined with 26.3 zinc are combined with 26.3 grams of hydrochloric acid?grams of hydrochloric acid?
Zn + 2 HCl Zn + 2 HCl ZnCl ZnCl22 + H + H22
15.5 g Zn x 1 mole Zn x 1 mole H2 x 22.4 L H2 = 5.31 L H2
65.4 g Zn 1 mole Zn 1 mole H2
26.3 g HCl x 1 mole HCl x 1 mole H2 x 22.4 L H2 = 8.07 L H2
36.5 g HCl 2 moles HCl 1 mole H2
Zn is the limiting reagent and 5.31 Liters of H2 are produced.
Reaction #5
Na + HNa + H22O O NaOH + H NaOH + H22
If 2.1g of sodium is added to 3.8g If 2.1g of sodium is added to 3.8g of water, what is the limiting of water, what is the limiting reagent, and how many grams of reagent, and how many grams of sodium hydroxide are produced?sodium hydroxide are produced?
2 Na + 2 H2 Na + 2 H22O O 2 NaOH + H 2 NaOH + H
22
2.1 g Na x 1 mole Na x 2 moles NaOH x 40 g NaOH = 3.7 g NaOH
23 g Na 2 moles Na 1 mole NaOH
3.8 g H2O x 1 mole H2O x 2 moles NaOH x 40 g NaOH = 8.4 g NaOH
18 g H2O 2 moles H2O 1 mole NaOH
Na is the limiting reagent and 3.7 g NaOH are produced.
In Review:In Review:
What is a limiting reagent?What is a limiting reagent?
What is the excess reagent?What is the excess reagent?
How does a limiting reagent control How does a limiting reagent control the amount of product?the amount of product?