Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a...
-
Upload
oscar-jasper-campbell -
Category
Documents
-
view
233 -
download
4
Transcript of Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a...
![Page 1: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/1.jpg)
Chemical Quantities and Moles
![Page 2: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/2.jpg)
Section 12.1
Counting Particles of Matter
• Define the mole as a counting number.
• Relate counting particles to weighing samples of substances.
• Solve stoichiometric problems using molar mass.
![Page 3: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/3.jpg)
Section 12.1
Counting Particles of Matter
Avogadro’s principle: equal volumes of gases at the same temperature and pressure contain equal numbers of particles
![Page 4: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/4.jpg)
Section 12.1
Counting Particles of Matter
stoichiometry
mole
Avogadro’s number
molar mass
molecular mass
formula mass
A mole always contains the same number of particles; however, moles of different substances have different masses.
![Page 5: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/5.jpg)
Section 12.1
• Stoichiometry is the study of quantitative relationships between reactants and products in a chemical reaction.
![Page 6: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/6.jpg)
Section 12.1
Stoichiometry (cont.)
• The group or unit of measure used to count number of atoms, molecules, ions, or formula units is the mole (abbreviated mol).
• The number of things in a mole is 6.02 × 1023 and is called Avogadro’s number.
![Page 7: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/7.jpg)
Section 12.1
Molar Mass• Using moles, macroscopic
measurements, such as mass, can be related to the molecules involved in a chemical reaction.
• The mass of one mole of a pure substance is called its molar mass.
![Page 8: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/8.jpg)
Section 12.1
Molar Mass (cont.)
• The molar mass of an element is simply the average atomic mass of that element stated in grams rather than atomic mass units.
![Page 9: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/9.jpg)
Section 12.1
Molar Mass (cont.)
• The molecular mass of a covalent compound is the mass in atomic mass units of one molecule.
– Its molar mass is the mass in grams of one mole of its molecules.
![Page 10: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/10.jpg)
Section 12.1
Molar Mass (cont.)
• The formula mass of an ionic compound is the mass in atomic mass units of one formula unit.
– Its molar mass is the mass in grams of one mole of its formula units.
![Page 11: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/11.jpg)
Section 12.1
Molar Mass and Stoichiometry
• The concept of molar mass makes it easy to determine the number of particles in a sample of a substance by simply measuring the mass of the sample.
• Use the molar mass to convert mass to moles or moles to mass.
![Page 12: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/12.jpg)
Section 12.2
Using Moles
• Predict quantities of reactants and products in chemical reactions.
• Determine mole ratios from formulas for compounds.
• Identify formulas of compounds by using mass ratios.
![Page 13: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/13.jpg)
Section 12.2
Using Moles
mole: group or unit of measure used to count numbers of atoms, molecules, or formula units of a substance
![Page 14: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/14.jpg)
Section 12.2
Using Moles
molar volume
ideal gas law
theoretical yield
percent yield
empirical formula
Balanced chemical equations relate moles of reactants to moles of products.
![Page 15: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/15.jpg)
Section 12.2
Using Molar Masses in Stoichiometric Problems
• Balanced chemical equations and moles can be used to predict the masses of reactants or products.
![Page 16: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/16.jpg)
Section 12.2
Using Molar Masses in Stoichiometric Problems (cont.)
![Page 17: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/17.jpg)
Section 12.2
Using Molar Volumes in Stoichiometric Problems
• The molar volume of a gas is the volume that a mole of gas occupies at a pressure of one atmosphere (equal to 101 kPa) and a temperature of 0.00°C.
![Page 18: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/18.jpg)
Section 12.2
• The ideal gas law describes the behavior of an ideal gas in terms of pressure (P), volume (V), temperature (T), and number of moles of gas, n.
PV = nRT (R represents the ideal gas constant)
Ideal Gas Law
![Page 19: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/19.jpg)
Section 12.2
• The amount of product of a chemical reaction predicted by stoichiometry is called the theoretical yield.
Theoretical Yield and Actual Yield
• The percent yield of a reaction is the ratio of the actual yield to the theoretical yield.
![Page 20: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/20.jpg)
• Percent composition of a compound can be determined from its chemical formula.
Determining Mass Percents
Composition of Geraniol
![Page 21: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/21.jpg)
Section 12.2
• To determine a chemical formula, find the relative numbers of each of the atoms in the formula unit of the compound.
Determining Chemical Formulas
• The formula of a compound having the smallest whole-number ratio of atoms in the compound is called the empirical formula.
![Page 22: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/22.jpg)
Section 12.2
Determining Chemical Formulas (cont.)
![Page 23: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/23.jpg)
Section 12.2
• The empirical formula of a compound can be determined from its percent composition.
• You can calculate the empirical formula from percent by mass by assuming you have 100.00 g of the compound. Then, convert to mass of each element to moles.
Determining Chemical Formulas
![Page 24: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/24.jpg)
Section 12.2
• Chemical formulas for most ionic compounds are the same as their empirical formulas.
• However, the empirical formula is not always the chemical formula.
Determining Chemical Formulas
![Page 25: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/25.jpg)
Section 12.2
• Many different covalent compounds have the same empirical formulas because atoms can share electrons in different ways.
• The chemical formula of a compound can be determined if the molar mass and the empirical formula are known.
Determining Chemical Formulas
![Page 26: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/26.jpg)
Key Concepts
• Stoichiometry relates the amounts of products and reactants in a chemical equation to one another.
• The mole is a unit used to count particles of matter. One mole of a pure substance contains Avogadro’s number of particles, 6.02 x 1023.
• Molar mass can be used to convert mass to moles or moles to mass.
![Page 27: Chemical Quantities and Moles Section 12.1 Counting Particles of Matter Define the mole as a counting number. Relate counting particles to weighing samples.](https://reader035.fdocuments.in/reader035/viewer/2022062217/56649e745503460f94b7530f/html5/thumbnails/27.jpg)
Key Concepts• A balanced chemical equation provides mole ratios of the
substances in the reaction.
• Percent composition can be determined from the chemical formula of a compound; the empirical formula of a compound can be determined from its percent composition.
• The chemical formula of a compound can be determined if the molar mass and the empirical formula are known.
• The ideal gas law is expressed in the following equation PV=nRT.
• Percent yield measures the efficiency of a chemical reaction.