Molar mass
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This document discusses molar mass and provides examples of calculating the molar mass of common compounds like sodium chloride, water, and aluminum sulfate. The molar mass of a substance is the mass of one mole of that substance. It demonstrates how to determine molar mass by adding up the atomic masses of each element in a compound's chemical formula based on the number of atoms present. Knowing molar mass allows one to measure out exactly one mole of a substance.
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- Chemical formulas indicate the types and numbers of atoms in a compound, which can be used to determine mole
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Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, consetetur sadipscing elitr, sed diam nonumy eirmod tempor invidunt ut labore et dolore magna aliquyam erat, sed diam voluptua. At vero eos et accusam et justo duo dolores et ea rebum. Stet clita kasd gubergren, no sea takimata sanctus est Lorem ipsum dolor sit amet. Lorem ipsum dolor sit amet, conset
The_Mole.ppt
This document provides information about the mole as a unit of measurement in chemistry. It defines the mole as a preferred unit used to represent small numbers of particles, such as atoms or molecules. The key points are:
- 1 mole is equal to 6.022 x 1023 representative particles, whether atoms, molecules, formula units, etc.
- Common mole-particle conversions include 1 mole of carbon = 12.011 g of carbon and 1 mole of any substance containing 6.022 x 1023 representative particles.
- Mole conversions can be used to determine the number of moles, grams, or particles between different units using dimensional analysis and provided conversion factors.
Ch 11 notes complete
The document discusses moles, molar mass, and empirical and molecular formulas.
It defines key terms like mole, Avogadro's number, and molar mass. A mole represents 6.02x1023 particles of a substance. Molar mass is the mass in grams of one mole of a substance.
Examples are provided for calculating moles from mass and vice versa using molar mass. Empirical formulas represent the lowest whole number ratio of elements in a compound, while molecular formulas specify the actual number of each atom in a molecule or formula unit.
Ch 11 notes complete
The document discusses moles, molar mass, and empirical and molecular formulas.
It defines key terms like mole, Avogadro's number, and molar mass. A mole represents 6.02x1023 particles of a substance. Molar mass is the mass in grams of one mole of a substance.
Examples are provided for calculating moles from mass and vice versa using molar mass. Empirical formulas give the lowest whole number ratio of elements in a compound, while molecular formulas specify the actual number of each atom in a molecule or formula unit.
THEMOLECONCEPT.pptx
This document discusses moles, molar mass, and Avogadro's number. It begins by asking questions about the number of particles in tablespoons of sugar and salt. It then provides background on Avogadro and defines Avogadro's number as 6.022x10^23 particles per mole. The document asks additional questions about moles, molar mass, atomic mass, and using calculations to determine the number of particles and moles in various substances.
Chapter8.ppt science 9*moleconceptslides
The document discusses the mole concept in chemistry. Some key points:
- 1 mole is equal to 6.02 x 1023 particles, whether atoms, molecules, ions, etc. This number is known as Avogadro's number.
- The mass of 1 mole of a substance in grams is equal to the substance's molar mass shown on the periodic table. For example, 1 mole of carbon is 12.01 g.
- Calculations can be done to convert between moles, mass, particles, and volume (at STP) using molar mass and Avogadro's number.
- Percent composition problems calculate the percentage of each element in a compound based on the
05a the mole
The document discusses the mole concept and related terms. It defines the mole as the unit used to count particles in chemistry and equals 6.022 x 1023 particles. It explains that one mole of an element equals its atomic mass in grams. Formula mass is the sum of atomic masses of elements in a formula unit, while molar mass refers to grams per mole of a pure substance. It provides examples of calculating moles, mass, and grams in chemical equations and reactions.
Conservation of Mass
Here are the steps to solve this practice problem:
A. C2H4 + 3O2 → 2CO2 + 2H2O
B. C2H4 = 28 g/mol, O2 = 32 g/mol, CO2 = 44 g/mol, H2O = 18 g/mol
C. If we want 2.25 mol CO2 and the ratio is 2:1, then we need 2.25 * 2 = 4.5 mol C2H4
4.5 mol C2H4 * 28 g/mol = 126 g of C2H4
D. The ratio of H2O to O2 is 2:3. If we have 12 g
Mole concept
The document discusses moles, molar mass, molar concentration, and stoichiometry. It defines a mole as 6.02 x 1023 particles, whether atoms, molecules, ions, or electrons. Molar mass is the mass of one mole of a substance in grams. Molar concentration, or molarity, expresses the moles of solute per liter of solution. Stoichiometry uses mole ratios from balanced chemical equations to calculate amounts of reactants and products.
3,stoichiometry
This document discusses stoichiometry, which is the quantitative study of chemical reactions. It defines key terms like atomic mass, isotopes, moles, molar mass, and percent composition. It provides examples of calculating these values, such as determining the number of atoms or moles of a substance based on its mass. The document establishes the relationships between atoms, moles, mass, and molar mass that are fundamental to stoichiometric calculations.
Final Review
1. The document discusses various stoichiometry concepts including mole-to-mole, mole-to-mass, and mass-to-mass calculations using balanced chemical equations.
2. Examples are provided for determining moles, grams, and numbers of particles from given values through step-by-step working.
3. Key stoichiometry topics covered are mole ratios, molar mass, percent composition, and solving various stoichiometric problems.
Stoichiometry
1. The concentrations given are: 1.0 E -9, 2.4 E -3, 6.7 E -7, 4.4 E -5.
2. The document discusses stoichiometry, mole conversions, molarity, and percent composition in chemistry.
3. Stoichiometry is the study of quantitative relationships in chemical reactions using molar ratios and mole conversions.
The mole
- A mole represents 6.02 x 10^23 particles of a substance, whether atoms, molecules, ions, etc. This number is known as Avogadro's number.
- Common examples are given to illustrate just how large Avogadro's number is, such as the number of atoms needed to cover the Earth's surface.
- The document provides examples of calculating the number of particles and moles of different substances.
Chemical Measurement (1).ppt
This document discusses the mole concept in chemistry. It defines atomic mass, formula mass, and molar mass. Atomic mass is a relative scale that compares atom masses to carbon-12. Formula mass is the sum of all atom masses in a compound. Molar mass is the mass in grams of one mole of a substance. A mole is defined as Avogadro's number (6.02x1023) of particles, which allows chemists to convert between number of particles and mass.
Chemistry - Chp 10 - Chemical Quantities - PowerPoint
This chapter discusses methods for measuring quantities of substances. It introduces the mole as a unit for measuring amounts of matter equal to Avogadro's number of representative particles. The mole allows for easy conversion between mass and number of particles. Compound formulas allow calculating formula mass in grams per mole. Relationships between moles, mass, and volume at standard temperature and pressure enable interconversion between these quantities.
Chapter 3 notes
The document defines atomic mass, molar mass, molecular mass, and formula mass. It explains that atomic mass is the mass of an atom measured in atomic mass units (amu) and is based on carbon-12. Molar mass is the mass of one mole of a substance in grams. One mole contains 6.022x1023 elementary units. Molecular mass is the sum of atomic masses in a molecule. Formula mass is the sum of atomic masses in a formula unit of an ionic compound. The document provides examples of calculating molar mass, molecular mass, and formula mass from atomic masses on the periodic table.
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Molar mass
- 2. Objective Measure out exactly 1 mole of a substance by determining the molar mass of some common compounds.
- 3. Molar mass The molar mass of a substance is the mass of 1 mole of that substance. Remember that 1 mole of a substance is equal to 6.02x1023 particles (atoms or molecules).
- 4. Molar mass - Sodium Chloride Sodium chloride: NaCl Atomic mass of Na: 22.99 x 1 atom of Na = 22.99 g/mol Atomic mass of Cl: 35.45 x 1 atom of Cl = 35.45 g/mol Molar mass of NaCl: 22.99 g/mol + 35.45 g/mol = 58.44 g/mol
- 5. Molar mass - Water Water: H2O Atomic mass of H: 1.01 x 2 atoms of H = 2.02 g/mol Atomic mass of O: 16.00 x 1 atom of O = 16.00 g/mol Molar mass of H2O: 2.02 g/mol + 16.00 g/mol = 18.02 g/mol
- 6. Molar mass - Aluminum sulfate Aluminum Sulfate: Al2(SO4)3 Atomic mass of Al: 26.98 x 2 atoms of Al = 53.96 g/mol Atomic mass of S: 32.06 x 3 atoms of S = 96.18 g/mol Atomic mass of O: 16.00 x 12 atoms of O = 192 g/mol Molar mass of Al2(SO4)3: 53.96 + 96.18 + 192 = 342.14 g/mol
- 7. Measure out exactly 1 mole of each of the compounds from the example Problems.
Editor's Notes
- Explain that 1 mole of one substance will more than likely have a molar mass that is different from other substances because different substances contain different atoms or different combinations of atoms or both.
- If time allows, practice the Molar Mass worksheet before the closing activity.
- Ideally, allow students to work in groups of three dividing the tasks evenly. To save time and money: omit the aluminum sulfate sample, but have a sample for the students to observe. This is the students’ exit ticket. Ask and evaluate: why is the mass of each sample significantly different in volume? As a challenge have students predict how many atoms of each type are found in each sample. I.e. the sample of sodium chloride has an approximate 6.02x1023 atoms of sodium and 6.02x1023 atoms of chlorine.