chapter 3 chemical stoichiometry. 3.1: atomic mass/weight the average mass of a sulfur atom is 32.06...
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Chapter 3
Chemical Stoichiometry
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3.1: Atomic Mass/Weight
The average mass of a sulfur atom is 32.06 amu
The average mass of a sodium atom is 22.99 amu
S
Na
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3.2: Molecular Mass/Weight Formula Mass/Weight
•The formula of an Acetylsalicylic Acid (Aspirin) molecule is C9H8O4
•Acetylsalicylic Acid (Aspirin) has molecular mass of 180.159 amu
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3.2: Molecular Mass/Weight Formula Mass/Weight
•Aluminum sulfate is an ionic compound with the formula Al2(SO4)3
•Aluminum sulfate has a formula mass of 342.153 amu.
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3.3: Isotopes
• Isotopes are atoms of an element that differ only in the number of neutrons in the nucleus of the atom.
• Chlorine has two isotopes:
chlorine – 35 35Cl
chlorine – 37 37Cl
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3.3: Isotopes
• In any random sample of chlorine about 1 in 4 atoms is chlorine – 37.
The atomic mass of chlorine is therefore about 35.5 amu.
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3.3: Isotopes
• How do atoms of chlorine – 35 and chlorine – 37 differ?
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3.4: Moles of Atoms and Avogadro’s Number
• What is a mole of atoms?
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3.4: Moles of Atoms and Avogadro’s Number
• What is a mole of atoms?
One mole of magnesium atoms contains
6.02 x 1023 Mg atoms.
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3.4: Moles of Atoms and Avogadro’s Number
• What is the mass of one mole of Mg atoms?
•The atomic mass of Mg is 24.305 amu.
•The molar mass of Mg is 24.305 grams.
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3.5: Moles of Molecules
• What is a mole of molecules?
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3.5: Moles of Molecules
• What is a mole of molecules?
• One mole of CHCl3 (chloroform) contains 6.02 x 1023 molecules of CHCl3.
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3.5: Moles of Molecules
• What is a mole of molecules?
• One mole of CHCl3 (chloroform) contains 6.02 x 1023 molecules of CHCl3.
• What else does it contain?
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3.5: Moles of Molecules
• How many H atoms are in one mole of CHCl3?
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3.5: Moles of Molecules
• How many H atoms are in one mole of CHCl3?
6.02 x 1023 H atoms
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3.5: Moles of Molecules
• How many Cl atoms are in one mole of CHCl3?
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3.5: Moles of Molecules
• How many Cl atoms are in one mole of CHCl3?
3(6.02 x 1023) Cl atoms
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3.5: Moles of Molecules
• What is the molar mass of CHCl3?
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3.5: Moles of Molecules
• What is the molar mass of CHCl3?
119.377g
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Key Concept
• You have one mole of ascorbic acid (Vitamin C) C6H8O6. What else do you have?
• 6.02 x 1023 molecules of C6H8O6
• 176.13 grams of C6H8O6
• 6 moles C or 6(6.02 x 1023) C atoms
• 8 moles H or 8(6.02 x 1023) H atoms
• 6 moles O or 6(6.02 x 1023) O atoms
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Key Concept
• If you have a certain number of moles of any compound you can always find the moles of each element present?
• How many mol C are in 0.80 mol of CO2?
• How many mol O are in 0.80 mol of CO2?
• How many mol H are in 1.2 mol of C12H22O11?
• How many mol S are in 3.8 mol of Cr(SO4)3?
• How many mol O are in 3.8 mol of Cr(SO4)3?
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3.6: Percentage Composition or Percent by Mass
•What is the percent by mass of hydrogen in water?
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3.6: Percentage Composition or Percent by Mass
A glass of water contains 126g of water. How many grams of hydrogen are present?
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3.7: Derivation of Formulas•To calculate a formula of a substance we often use a mole ratio.
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3.7: Derivation of Formulas•To calculate a formula of a substance we often use a mole ratio.Analysis of a gas shows that it is composed of 0.090 mol carbon and 0.36 mol hydrogen. What is the empirical formula gas?
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3.7: Derivation of Formulas
What is the empirical formula of a compound that is 27.29% carbon and 72.71% oxygen.
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3.7: Derivation of FormulasA sample of hematite contains 34.97g of iron and 15.03g of oxygen. What is the empirical formula of hematite?
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Determine the empirical and molecular formulas for a compound with the following elemental composition: 40.00% C, 6.72% H, 53.29% O. The molar mass of the compound is 180. g/mol.
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Determine the empirical and molecular formulas for a compound with the following elemental composition: 40.00% C, 6.72% H, 53.29% O. The molar mass of the compound is 180. g/mol.
C mol 3.331 C g 12.01
C mol 1 x C g 40.00
H mol 6.667 H g 1.008
H mol 1 x H g 6.72
O mol 3.331 O g 16.00
O mol 1 x O g 53.29
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Determine the empirical and molecular formulas for a compound with the following elemental composition: 40.00% C, 6.72% H, 53.29% O. The molar mass of the compound is 180. g/mol.
C 1 C 1.000 mol 3.331
C mol 3.331
H 2 H 2.001 mol 3.331
H mol 6.667
O 1 O 1.000 mol 3.331
O mol 3.331
CH2O
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Determine the empirical and molecular formulas for a compound with the following elemental composition: 40.00% C, 6.72% H, 53.29% O. The molar mass of the compound is 180. g/mol.
CH2O
• 12.01 + 2(1.008) + 1 (16.00) = 30.03
• 180./30.03 ≈ 6
• 6(CH2O) = C6H12O6
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3.7: Derivation of Formulas
3.22g of a compound decomposes when heated into 1.96g of KCl and oxygen. What is the empirical formula of the compound?
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3.8: Solutions
• Solute: The substance that dissolves (the minor component of a solution).
KMnO4
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3.8: Solutions
• Solvent: The substance in which the solute dissolves (the major component of a solution).
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KMnO4 solution
Solution: A homogeneous mixture of the solute and solvent.
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3.8: Solutions
Dilute Concentrated
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Concentration of a solution
Molarity(M) is the moles of solute per liter of solution.
Molarity(M) =moles of soluteLiters of solution
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Preparation of Solutions
28.3 grams of nickel(II) chloride
Add water to make the desired volume (500.0 ml)
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Molarity
• Calculate the molarity of an aqueous nickel (II) chloride solution containing 28.3 grams of nickel (II) chloride in 500.0 mL of solution.
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Molarity The maximum solubility of lead (II)
chromate, PbCrO4, is 4.3 x 10-5 g/L. What is the molarity of a saturated solution of PbCrO4?
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Molarity How many moles of sulfuric acid, H2SO4, are contained in 0.80L of a 0.050M solution of sulfuric acid?
How many grams of H2SO4 would be needed to make this solution?
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Dilution• If we take a more concentrated solution we can dilute
it to a lower concentration by adding water to it.
• We determine the concentration (molarity) of the diluted solution by using the following formula.
M1V1 = M2V2
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Dilution• Calculate the concentration of the resulting solution
when enough water is added to 250.0mL of 0.60M NaOH to make 300.0mL of solution?
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Dilution• How much water would need to be added to 125mL of
a 1.50M solution of HCl to dilute the solution to a concentration of 0.570M?
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Density
• An understanding of density is often necessary in solving various problems.
• Density is a ratio of mass to volume and therefore can be used in the conversion of mass to volume or volume to mass.
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Mass Percent
• An understanding of mass percent is often necessary in solving various problems.
• Mass percent indicates the percentage of a particular substance in a mixture.
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Aniline, C6H5NH2, a key ingredient in the preparation of dyes for fabrics, is produced by the reaction of C6H5Cl with a solution containing 28.2% NH3 by mass. If the density of the NH3 solution is 0.899g/cm3. What mass of NH3 is needed to prepare 125mL of
the ammonia solution?
aniline
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Aniline, C6H5NH2, a key ingredient in the preparation of dyes for fabrics, is produced by the reaction of C6H5Cl with a solution containing 28.2% NH3 by mass. If the density of the NH3 solution is 0.899g/cm3. What mass of NH3 is needed to prepare 125mL of
the ammonia solution?
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Stoichiometry: Calculations based on balanced equations.
• We use the balanced equation to determine a mole ratio.
• Then we use “Moles to Move”.
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Stoichiometry: Calculations based on balanced equations.
How many moles of Al2I6 are produced from 0.40 mol Al?
+ →
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Stoichiometry: Calculations based on balanced equations.
Calculate the moles of oxygen produced by the thermal decomposition of 100.0g of potassium chlorate.
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Stoichiometry: Calculations based on balanced equations.
Calculate the moles of oxygen produced by the thermal decomposition of 100.0g of potassium chlorate.
• Write the equation for this reaction.
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Calculate the moles of oxygen produced by the thermal decomposition of 100.0g of potassium chlorate.
• Write the equation for this reaction.
2KClO3 → 2KCl + 3O2
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Calculate the moles of oxygen produced by the thermal decomposition of 100.0g of potassium chlorate.
2KClO3 → 2KCl + 3O2
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• The antacid milk of magnesia contains Mg(OH)2. What mass of NaOH would be needed to produce 16g of Mg(OH)2? MgCl2 + 2NaOH → Mg(OH)2 + 2NaCl
.
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• The antacid milk of magnesia contains Mg(OH)2. What mass of NaOH would be needed to produce 16g of Mg(OH)2?
MgCl2 + 2NaOH → Mg(OH)2 + 2NaCl
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What mass of oxygen is required to burn 702g of octane?
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What mass of oxygen is required to burn 702g of octane?Write the balanced equation for this reaction.
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What mass of oxygen is required to burn 702g of octane?2C8H18 + 25O2 → 16CO2 + 18H2O
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•What volume of 0.750M HCl can be made from 25.0g of NaCl?
NaCl + H2SO4 → HCl + NaHSO4
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•What volume of 0.2089M KI solution reacts with 43.88mL of 0.3842M Cu(NO3)2?
2Cu(NO3)2 + 4KI → 2CuI + I2 + 4KNO3
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Percentage Yield
Percent Yield = actual yieldtheoretical yield
X 100
Percentage yield can be a part of stoichiometry problems
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Percentage Yield
• 1.274g of CuSO4 produces 0.392g of Cu. What is the percentage yield?
CuSO4 + Zn → Cu + ZnSO4
→
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Percentage Yield
• 1.274g of CuSO4 produces 0.392g of Cu. What is the percentage yield?
CuSO4 + Zn → Cu + ZnSO4
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Limiting Reagents
• A limiting reagent (reactant) is the reactant that is used up in a chemical reaction.
• All other reactants are said to be in excess.
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Limiting Reagent
• 195g NaHCO3 and 152ml 3.0M HC2H3O2
NaHCO3 + HC2H3O2 → NaC2H3O2 + H2CO3
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Limiting Reagent
• 195g NaHCO3 and 152ml 3.0M HC2H3O2
NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2
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Limiting Reagent
• 195g NaHCO3 and 152ml 3.0M HC2H3O2
• Which reactant is limiting?
NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2
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Limiting Reagent
• 195g NaHCO3 and 152ml 3.0M HC2H3O2
• Which reactant is limiting?
• How many grams of CO2 are produced?
NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2
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Limiting Reagent
• 195g NaHCO3 and 152ml 3.0M HC2H3O2
• Which reactant is limiting?
• How many grams of CO2 are produced?
• How many grams of NaHCO3 remain after the reaction?
NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2
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Limiting Reagent
• 195g NaHCO3 and 152ml 3.0M HC2H3O2
• How many grams of NaHCO3 remain after the reaction?
NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2
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A mixture of 5.0g H2 and 10.0g of O2 is ignited forming water. How much water will the reaction produce?
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Titration• Titration is a common laboratory method of quantitative
chemical analysis that is used to determine the unknown concentration of a reactant.
• Because volume measurements play a key role in titration, it is also known as volumetric analysis.
• A reagent, called the titrant, is placed in a calibrated buret and reacted with another solution.
• One of the solutions is of known concentration (a standard solution). It is used to react with a solution whose concentration is not known.
• An indicator is used to identify the endpoint of the reaction. The point at which the reaction is complete. The endpoint is often indicated by a permanent change in color due to the indicator.
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Titration
Before endpoint
Endpoint
Overshoot
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Titration (Acid – Base)
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0.5105g NaOH is dissolved in water and titrated to an endpoint with 48.47 mL of HCl. What is the concentration of HCl?
NaOH + HCl → NaCl + H2O
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A solution of 20.00mL of oxalic acid was titrated to an endpoint with 23.23mL of 0.09113M potassium permanganate. What is the
concentration of the oxalic acid solution.
5H2C2O4 + 2KMnO4 + 3H2SO4 → 2MnSO4 + K2SO4 + 10CO2 + 8H2O
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How many grams of a sample containing 75.0% calcium hydroxide by mass is required to react with the acetic acid in 25.0mL of a solution having a density of 1.065 g/mL and
containing 58.0% acetic acid by mass?
Ca(OH)2 + 2HC2H3O2 → Ca(C2H3O2)2 + 2H2O