Calculating Moles.pptx
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The document discusses the mole, which is defined as 6.022x1023 particles and is used as a unit to describe large numbers of atoms or molecules. It explains that the molar mass of a substance is the mass in grams of one mole of that substance, and provides examples of calculating the number of moles and particles for given masses of various elements and compounds. The document also demonstrates how to use the mole concept to convert between mass and number of particles.
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7648568.ppt
1) The document discusses moles, Avogadro's number, and molar mass. It defines a mole as 6.02 x 1023 particles, such as atoms, ions, or molecules.
2) To convert between moles and particles, atoms, or molecules, you must multiply or divide by Avogadro's number. Molar mass is the mass in grams of one mole of a substance and is used to convert between moles and grams.
3) Examples are provided for calculating molar mass and for converting between moles, grams, and number of particles using molar mass and Avogadro's number.
Mole Concept.pptx (Grade 9, second quarter)
The document discusses the mole concept in chemistry. It defines the mole as the amount of substance that contains as many elementary units (atoms, molecules, ions) as there are atoms in exactly 12 grams of carbon-12. The number of elementary units in one mole is Avogadro's number, which is approximately 6.022x1023. Examples are given to illustrate that one mole of any substance will contain this number of particles, though the masses in grams will vary depending on the molar masses of the substances. The mole can be used to convert between the number of particles, moles, and mass in grams for calculations involving chemical substances.
basic concepts of chemistry
This document provides an overview of basic chemistry concepts including:
- Dalton's atomic theory and modern atomic theory which established atoms as the fundamental units of matter and that they can exist as isotopes.
- Berzelius hypothesis and Avogadro's law which established that equal volumes of gases under similar conditions contain equal numbers of molecules.
- Definitions of atoms, molecules, atomic mass, molecular mass, gram atomic mass, gram molecular mass, formula mass, and gram formula mass.
- Introduction of the mole concept based on Avogadro's number, which established a mole as a specific number of particles (atoms or molecules).
Mole Concept
- The mole concept allows chemists to conveniently keep track of large numbers of particles. A mole is defined as 6.02 x 1023 particles, whether atoms, molecules, ions, etc.
- The formula mass (or molar mass) of a compound is the sum of the atomic masses of each element in its chemical formula. It has units of grams per mole (g/mol).
- Calculations involving moles, mass, particles and formula mass allow conversions between the microscopic and macroscopic scales in chemistry.
Moles
The document discusses moles, which are a unit used to measure very large quantities in chemistry. A mole is defined as 6.02 x 1023 particles, such as atoms, molecules, ions. This number is known as Avogadro's number. The document provides examples of how many everyday items would equal a mole to demonstrate just how large a mole is. It also discusses how moles can be used to convert between the number of particles, moles, and mass in grams.
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.
Unit 4 cp the molef
The document provides instructions for calculating the empirical formula from percent composition data. It explains that the empirical formula represents the simplest whole number ratio of elements in a compound. The steps outlined are: 1) Convert the percentage of each element to grams. 2) Calculate the moles of each element using molar mass conversion factors. 3) Divide each mole value by the smallest mole value to determine the simplest mole ratio. 4) Multiply the ratios by the smallest number if needed to obtain whole numbers. An example problem is provided to demonstrate calculating the empirical formula of methyl acetate from its given percent composition.
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This document defines key concepts related to atoms and isotopes, including:
- Atomic number determines the identity of an element and is equal to the number of protons and electrons. Isotopes of an element can have different numbers of neutrons.
- Mass number is the total number of protons and neutrons in an isotope's nucleus.
- The mole is the amount of substance containing as many elementary entities as there are atoms in 12 grams of carbon-12, whose value is Avogadro's number, 6.022x1023.
- Molar mass is the mass of one mole of a substance and is numerically equal to the atomic mass of an element in grams per mole (g/mol).
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7648568.ppt
1) The document discusses moles, Avogadro's number, and molar mass. It defines a mole as 6.02 x 1023 particles, such as atoms, ions, or molecules.
2) To convert between moles and particles, atoms, or molecules, you must multiply or divide by Avogadro's number. Molar mass is the mass in grams of one mole of a substance and is used to convert between moles and grams.
3) Examples are provided for calculating molar mass and for converting between moles, grams, and number of particles using molar mass and Avogadro's number.
Mole Concept.pptx (Grade 9, second quarter)
The document discusses the mole concept in chemistry. It defines the mole as the amount of substance that contains as many elementary units (atoms, molecules, ions) as there are atoms in exactly 12 grams of carbon-12. The number of elementary units in one mole is Avogadro's number, which is approximately 6.022x1023. Examples are given to illustrate that one mole of any substance will contain this number of particles, though the masses in grams will vary depending on the molar masses of the substances. The mole can be used to convert between the number of particles, moles, and mass in grams for calculations involving chemical substances.
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This document provides an overview of basic chemistry concepts including:
- Dalton's atomic theory and modern atomic theory which established atoms as the fundamental units of matter and that they can exist as isotopes.
- Berzelius hypothesis and Avogadro's law which established that equal volumes of gases under similar conditions contain equal numbers of molecules.
- Definitions of atoms, molecules, atomic mass, molecular mass, gram atomic mass, gram molecular mass, formula mass, and gram formula mass.
- Introduction of the mole concept based on Avogadro's number, which established a mole as a specific number of particles (atoms or molecules).
Mole Concept
- The mole concept allows chemists to conveniently keep track of large numbers of particles. A mole is defined as 6.02 x 1023 particles, whether atoms, molecules, ions, etc.
- The formula mass (or molar mass) of a compound is the sum of the atomic masses of each element in its chemical formula. It has units of grams per mole (g/mol).
- Calculations involving moles, mass, particles and formula mass allow conversions between the microscopic and macroscopic scales in chemistry.
Moles
The document discusses moles, which are a unit used to measure very large quantities in chemistry. A mole is defined as 6.02 x 1023 particles, such as atoms, molecules, ions. This number is known as Avogadro's number. The document provides examples of how many everyday items would equal a mole to demonstrate just how large a mole is. It also discusses how moles can be used to convert between the number of particles, moles, and mass in grams.
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.
Unit 4 cp the molef
The document provides instructions for calculating the empirical formula from percent composition data. It explains that the empirical formula represents the simplest whole number ratio of elements in a compound. The steps outlined are: 1) Convert the percentage of each element to grams. 2) Calculate the moles of each element using molar mass conversion factors. 3) Divide each mole value by the smallest mole value to determine the simplest mole ratio. 4) Multiply the ratios by the smallest number if needed to obtain whole numbers. An example problem is provided to demonstrate calculating the empirical formula of methyl acetate from its given percent composition.
Chapter 3.3 : Counting Atoms
This document defines key concepts related to atoms and isotopes, including:
- Atomic number determines the identity of an element and is equal to the number of protons and electrons. Isotopes of an element can have different numbers of neutrons.
- Mass number is the total number of protons and neutrons in an isotope's nucleus.
- The mole is the amount of substance containing as many elementary entities as there are atoms in 12 grams of carbon-12, whose value is Avogadro's number, 6.022x1023.
- Molar mass is the mass of one mole of a substance and is numerically equal to the atomic mass of an element in grams per mole (g/mol).
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Concept of mole
1. A mole is defined as the amount of substance containing 6.02 x 1023 particles and can refer to atoms, molecules, or ions.
2. The mole is the unit for quantifying amount of substance, with the symbol "mol".
3. The number of particles in a given number of moles can be calculated by multiplying the moles by Avogadro's number, and the moles for a given number of particles is calculated by dividing the particles by Avogadro's number.
Student Ch 9 The Mole
The document provides information about moles, Avogadro's number, molar mass, and stoichiometry calculations. It defines the mole as the unit for counting particles, explains that one mole contains 6.02 x 1023 particles, and how this relates to molar mass. It gives examples of calculating moles, grams, and atoms/molecules using molar mass and stoichiometric conversions through mole ratios.
Ch 10 PPT...The Mole.pptx
This document discusses different methods of measuring matter, including counting, mass, and volume. It then explains how to convert between units using the factor-label method. A mole is defined as 6.02x1023 representative particles of an element or compound. The mass of one mole of a substance is called its molar mass. Molar mass can be used to convert between moles and grams. The volume of one mole of gas at standard temperature and pressure is 22.4 L.
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This document discusses atomic mass, molar mass, moles, and Avogadro's number. It defines a mole as the amount of substance containing as many elementary entities as there are atoms in exactly 12 grams of carbon-12. Molar mass is the mass in grams of one mole of a substance. Avogadro's number is the number of particles in one mole of a substance, which is 6.022x1023. Examples are provided for calculating mass from moles and number of atoms from moles using molar mass, moles, and Avogadro's number. Practice problems with solutions are included at the end.
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The document discusses the mole concept in chemistry. It defines the mole as the amount of a substance that contains as many elementary entities (atoms, molecules, ions, etc.) as there are atoms in exactly 12 grams of carbon-12. This number is known as Avogadro's number and is equal to 6.022×1023. The mole allows chemists to convert between the mass of a sample and the number of particles it contains. It provides a link between macroscopic and microscopic scales in chemistry. The mole is a central unit for quantitative chemical calculations and experiments.
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The document discusses the concept of the mole in chemistry. It defines a mole as 6.02 x 1023 representative particles, which can be atoms, molecules, or formula units. It provides examples of calculating the number of moles and mass of different substances. It also explains that 1 mole of any gas occupies 22.4 liters at standard temperature and pressure. Key terms discussed include molar mass, percent composition, empirical formula, and molecular formula.
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The document discusses the mole concept in chemistry. Some key points include:
- The mole represents a counted number of particles and in chemistry represents 6.02 x 1023 particles, known as Avogadro's number.
- Common calculations involving moles include converting between moles and number of particles/atoms/molecules, moles and mass using molar mass, and moles and volume at standard temperature and pressure.
- Molar mass is the mass in grams of one mole of a substance and is calculated by adding the atomic masses from the periodic table based on the chemical formula.
- Chemical formulas indicate the types and numbers of atoms in a compound, which can be used to determine mole
Chemunit9presentation 120212132140-phpapp01
- The mole is used to indirectly count particles of matter and relates to Avogadro's number of 6.022x10^23 particles.
- A mole of any pure substance, whether an element or compound, has a mass in grams equal to its molar mass.
- Molar mass can be used to convert between moles of a substance and its mass in grams.
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The document discusses the mole concept in chemistry. It defines one mole as 6.02 x 1023 particles, such as atoms or molecules. It also defines one mole of carbon-12 atoms as having a mass of exactly 12 grams. The document provides examples of using the mole concept to convert between moles, mass in grams, number of particles, and volume of gases.
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The document discusses the mole concept and how it allows chemists to quantify matter by counting particles using Avogadro's number rather than mass alone. It explains how the mole is defined as 6.022x10^23 particles and can be used to determine the number of atoms in a sample by calculating the number of moles and multiplying by Avogadro's number. Examples are provided to illustrate how to perform mole calculations and determine the number of particles in a chemical substance.
This activity is designed to introduce a convenient unit used by.docx
This activity is designed to introduce a convenient unit used by chemists and to illustrate uses of the unit.
Part I: What Is a Mole And Why Are Chemists Interested in It?
Counting things is a normal part of everyday life. How many days left until vacation? How many eggs do I need for the recipe? If large numbers of things are involved, we use grouping
strategies to make the numbers easier to manage. For example, 4 more
weeks
until vacation, tells
us that there are twenty-eight days. One
dozen
eggs is the common way of expressing the quantity
12.
Half of a dozen of anything would be 6 units. One
gross
is 144 items (12 dozen) and a
ream
of paper contain 500 sheets.
Chemist are faced with a unique problem when dealing with numbers of atoms or molecules. The particles are so small that any amount of them that we are able to physically handle contains a number of particles so large that there is nothing else in our experience that contains so many units. This
incredibly
large number calls for a special counting group -
the MOLE.
A
MOLE
is
6.022
x
1023
particles
. This is often referred to as
Avogadro=s
number
. Let=s make sure we understand how big this is. One mole of the element carbon has a mass of 12.01 grams. The smallest particle of an element is an atom. So one mole of carbon contains 602,200,000,000,000,000,000,000 atoms of carbon.
Look for the element carbon on the periodic table. Do you notice anything special about the value 12.01? Explain
The mass of one mole of the element magnesium is 24.30 grams. How many atoms does a sample of magnesium with a mass of 24.30 grams contain?
Stated in general terms, the mass of one mole of any element is equal to the
of that element expressed in grams. The mass of a mole of any element can be found by looking on .
The mass of 0.5000 moles of carbon is and contains
atoms of carbon.
Remember when dividing numbers written in scientific notation the number portion is divided
normally and the exponents are subtracted.
6.022x1023
divided by 2 is the same as 6.022 x1023/2
x
100.
So the answer is found by dividing 6.022 by 2 = 3.011 and the subtracting exponent 0
from exponent 23.
The answer in scientific notation is 3.011x1023
atoms
of carbon.
Calculator tip
: for exponential notation use the EE or EXP key (not 10^)
If you have a bottle containing 8.10 grams of magnesium, how many Mg atoms are present in the bottle? Show your work. What is different about this problem compared to the last one involving carbon?
Remember that some elements, when alone, exist in the form of diatomic molecules: H2, O2, N2, I2, F2, Cl2, Br2, Their smallest piece is a molecule containing two atoms. If one mole of oxygen were required for an experiment you would be using O2 the gas. One mole of O2 would have a mass of
and contain particles (molecules).
The characteristic unit of the compound CO2 is a molecule. Each CO2 molecule has atoms. In order to find the mass .
Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
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Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
INTRODUCTION
MORE ABOUT MOLE
WHAT IS THE MOLE CONCEPT?
MORE ABOUT MOLE CONCEPT
RELATIONSHIP BETWEEN MOLE, AVOGADRO NUMBER, AND MASS
AVOGADRO NUMBER
FEW MORE EXAMPLES
Every topic of this chapter is well written concisely and visuals will help you in understanding and imagining the practicality of all the topics.
By Shivam Parmar (PPT Designer)
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The document provides an introduction to stoichiometry and the mole concept. It discusses key topics including:
1. The mole is a unit used to describe the amount of substance in chemistry and is equal to 6.022x1023 particles.
2. The molar mass of an element or compound is the mass in grams of one mole and can be used to calculate amounts in chemical reactions.
3. Conversions can be made between moles, particles, masses, and volumes using the molar mass and molar relationships like moles = mass/molar mass.
4. Solution concentration is expressed in molarity, which is the moles of solute per liter of solution. M
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The document defines key chemistry concepts related to moles, including:
- A mole refers to Avogadro's number (6.02x10^23) of particles like atoms, molecules, ions or formula units.
- 1 mole of an element contains 6.02x10^23 atoms, 1 mole of a molecular compound contains 6.02x10^23 molecules, and 1 mole of an ionic compound contains 6.02x10^23 formula units.
- Gram atomic mass refers to the mass of one mole of an element in grams, and gram formula mass refers to the sum of atomic weights that make up one mole of a compound.
- Chemical formulas represent the
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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.
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This document discusses quantitative chemistry concepts including the mole, Avogadro's constant, molar mass, and using moles to calculate the number of particles and mass of substances. Some key points covered are:
- A mole is a unit used to count fundamental particles and represents 6.02x1023 particles.
- The mole allows converting between large numbers of particles and more manageable units like grams.
- Molar mass relates the mass of a sample of a substance to the number of moles it contains.
- Problems use molar mass to calculate moles, particles, or mass given any two of those quantities.
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Concept of mole
1. A mole is defined as the amount of substance containing 6.02 x 1023 particles and can refer to atoms, molecules, or ions.
2. The mole is the unit for quantifying amount of substance, with the symbol "mol".
3. The number of particles in a given number of moles can be calculated by multiplying the moles by Avogadro's number, and the moles for a given number of particles is calculated by dividing the particles by Avogadro's number.
Student Ch 9 The Mole
The document provides information about moles, Avogadro's number, molar mass, and stoichiometry calculations. It defines the mole as the unit for counting particles, explains that one mole contains 6.02 x 1023 particles, and how this relates to molar mass. It gives examples of calculating moles, grams, and atoms/molecules using molar mass and stoichiometric conversions through mole ratios.
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This document discusses different methods of measuring matter, including counting, mass, and volume. It then explains how to convert between units using the factor-label method. A mole is defined as 6.02x1023 representative particles of an element or compound. The mass of one mole of a substance is called its molar mass. Molar mass can be used to convert between moles and grams. The volume of one mole of gas at standard temperature and pressure is 22.4 L.
Applied Chapter 3.4 : Counting Atoms
This document discusses atomic mass, molar mass, moles, and Avogadro's number. It defines a mole as the amount of substance containing as many elementary entities as there are atoms in exactly 12 grams of carbon-12. Molar mass is the mass in grams of one mole of a substance. Avogadro's number is the number of particles in one mole of a substance, which is 6.022x1023. Examples are provided for calculating mass from moles and number of atoms from moles using molar mass, moles, and Avogadro's number. Practice problems with solutions are included at the end.
Class 11 sbcc part VI
The document discusses the mole concept in chemistry. It defines the mole as the amount of a substance that contains as many elementary entities (atoms, molecules, ions, etc.) as there are atoms in exactly 12 grams of carbon-12. This number is known as Avogadro's number and is equal to 6.022×1023. The mole allows chemists to convert between the mass of a sample and the number of particles it contains. It provides a link between macroscopic and microscopic scales in chemistry. The mole is a central unit for quantitative chemical calculations and experiments.
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The document discusses the concept of the mole in chemistry. It defines a mole as 6.02 x 1023 representative particles, which can be atoms, molecules, or formula units. It provides examples of calculating the number of moles and mass of different substances. It also explains that 1 mole of any gas occupies 22.4 liters at standard temperature and pressure. Key terms discussed include molar mass, percent composition, empirical formula, and molecular formula.
Ch 11 notes complete
The document discusses the mole concept in chemistry. Some key points include:
- The mole represents a counted number of particles and in chemistry represents 6.02 x 1023 particles, known as Avogadro's number.
- Common calculations involving moles include converting between moles and number of particles/atoms/molecules, moles and mass using molar mass, and moles and volume at standard temperature and pressure.
- Molar mass is the mass in grams of one mole of a substance and is calculated by adding the atomic masses from the periodic table based on the chemical formula.
- Chemical formulas indicate the types and numbers of atoms in a compound, which can be used to determine mole
Chemunit9presentation 120212132140-phpapp01
- The mole is used to indirectly count particles of matter and relates to Avogadro's number of 6.022x10^23 particles.
- A mole of any pure substance, whether an element or compound, has a mass in grams equal to its molar mass.
- Molar mass can be used to convert between moles of a substance and its mass in grams.
The mole (2)
The document discusses the mole concept in chemistry. It defines one mole as 6.02 x 1023 particles, such as atoms or molecules. It also defines one mole of carbon-12 atoms as having a mass of exactly 12 grams. The document provides examples of using the mole concept to convert between moles, mass in grams, number of particles, and volume of gases.
MOLES science9
The document discusses the mole concept and how it allows chemists to quantify matter by counting particles using Avogadro's number rather than mass alone. It explains how the mole is defined as 6.022x10^23 particles and can be used to determine the number of atoms in a sample by calculating the number of moles and multiplying by Avogadro's number. Examples are provided to illustrate how to perform mole calculations and determine the number of particles in a chemical substance.
This activity is designed to introduce a convenient unit used by.docx
This activity is designed to introduce a convenient unit used by chemists and to illustrate uses of the unit.
Part I: What Is a Mole And Why Are Chemists Interested in It?
Counting things is a normal part of everyday life. How many days left until vacation? How many eggs do I need for the recipe? If large numbers of things are involved, we use grouping
strategies to make the numbers easier to manage. For example, 4 more
weeks
until vacation, tells
us that there are twenty-eight days. One
dozen
eggs is the common way of expressing the quantity
12.
Half of a dozen of anything would be 6 units. One
gross
is 144 items (12 dozen) and a
ream
of paper contain 500 sheets.
Chemist are faced with a unique problem when dealing with numbers of atoms or molecules. The particles are so small that any amount of them that we are able to physically handle contains a number of particles so large that there is nothing else in our experience that contains so many units. This
incredibly
large number calls for a special counting group -
the MOLE.
A
MOLE
is
6.022
x
1023
particles
. This is often referred to as
Avogadro=s
number
. Let=s make sure we understand how big this is. One mole of the element carbon has a mass of 12.01 grams. The smallest particle of an element is an atom. So one mole of carbon contains 602,200,000,000,000,000,000,000 atoms of carbon.
Look for the element carbon on the periodic table. Do you notice anything special about the value 12.01? Explain
The mass of one mole of the element magnesium is 24.30 grams. How many atoms does a sample of magnesium with a mass of 24.30 grams contain?
Stated in general terms, the mass of one mole of any element is equal to the
of that element expressed in grams. The mass of a mole of any element can be found by looking on .
The mass of 0.5000 moles of carbon is and contains
atoms of carbon.
Remember when dividing numbers written in scientific notation the number portion is divided
normally and the exponents are subtracted.
6.022x1023
divided by 2 is the same as 6.022 x1023/2
x
100.
So the answer is found by dividing 6.022 by 2 = 3.011 and the subtracting exponent 0
from exponent 23.
The answer in scientific notation is 3.011x1023
atoms
of carbon.
Calculator tip
: for exponential notation use the EE or EXP key (not 10^)
If you have a bottle containing 8.10 grams of magnesium, how many Mg atoms are present in the bottle? Show your work. What is different about this problem compared to the last one involving carbon?
Remember that some elements, when alone, exist in the form of diatomic molecules: H2, O2, N2, I2, F2, Cl2, Br2, Their smallest piece is a molecule containing two atoms. If one mole of oxygen were required for an experiment you would be using O2 the gas. One mole of O2 would have a mass of
and contain particles (molecules).
The characteristic unit of the compound CO2 is a molecule. Each CO2 molecule has atoms. In order to find the mass .
Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
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Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
INTRODUCTION
MORE ABOUT MOLE
WHAT IS THE MOLE CONCEPT?
MORE ABOUT MOLE CONCEPT
RELATIONSHIP BETWEEN MOLE, AVOGADRO NUMBER, AND MASS
AVOGADRO NUMBER
FEW MORE EXAMPLES
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CHEMISTRY CHAPTER 1.2 Mole Concepts.pptx
The document discusses various mole concepts including:
- Defining the mole and Avogadro's constant.
- Relating moles, mass, and particles for elements, compounds, and ions.
- Calculating molar mass and mass from moles.
- Relating the volume of gases to moles using Avogadro's law and molar volume.
- Explaining empirical and molecular formulas and calculating them from composition data.
- Defining different concentration units - molarity, molality, mole fraction, percentage by mass and volume.
Cw stoichiometry intro 041112
The document provides an introduction to stoichiometry and the mole concept. It discusses key topics including:
1. The mole is a unit used to describe the amount of substance in chemistry and is equal to 6.022x1023 particles.
2. The molar mass of an element or compound is the mass in grams of one mole and can be used to calculate amounts in chemical reactions.
3. Conversions can be made between moles, particles, masses, and volumes using the molar mass and molar relationships like moles = mass/molar mass.
4. Solution concentration is expressed in molarity, which is the moles of solute per liter of solution. M
c4e237864d12cdb0be66e0e86247e4cben4.pptx
Mole concept it's explanation and calculations on mole concept including concentration.
MOLE; Avogadro's Number; Percentage Composition
The document defines key chemistry concepts related to moles, including:
- A mole refers to Avogadro's number (6.02x10^23) of particles like atoms, molecules, ions or formula units.
- 1 mole of an element contains 6.02x10^23 atoms, 1 mole of a molecular compound contains 6.02x10^23 molecules, and 1 mole of an ionic compound contains 6.02x10^23 formula units.
- Gram atomic mass refers to the mass of one mole of an element in grams, and gram formula mass refers to the sum of atomic weights that make up one mole of a compound.
- Chemical formulas represent the
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.
2016 topic 01 part 1
This document discusses quantitative chemistry concepts including the mole, Avogadro's constant, molar mass, and using moles to calculate the number of particles and mass of substances. Some key points covered are:
- A mole is a unit used to count fundamental particles and represents 6.02x1023 particles.
- The mole allows converting between large numbers of particles and more manageable units like grams.
- Molar mass relates the mass of a sample of a substance to the number of moles it contains.
- Problems use molar mass to calculate moles, particles, or mass given any two of those quantities.
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Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
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Calculating Moles.pptx
- 1. Mole and Number of Moles of a Given Compound MRS. CYRIL A. CONSTANTINO
- 3. Atom is the basic unit of an element. According to John Dalton, atom was extremely small and indivisible. Can you count the atoms?
- 4. Atomic mass unit - unit provides relative scale for the masses of elements. Chemist used a special unit to describe a very large number of atoms. mole (mol) 1 mole = 6.022 x 1023 particles. This number is called the Avogadro’s number in honor of Italian scientist named Amadeo Avogadro. a pair means 2 (two) a dozen means 12 (twelve) a gross means 144 items.
- 5. Mole Mole is the amount of a substance that contains particles. These particles can be an atom, a molecule, an ion. One mole is said to be the number of atoms in exactly 12 grams of the isotope 12C It is also defined as the amount of substance containing the Avogadro’s number in any kind of chemical unit.
- 6. Mole The mass in grams of one mole of substance called molar mass. For example, •1 mole of C12 atom = 12 grams = 6.022 x 1023 atoms. Element Atomic Weight Molar Mass Avogadro’s Number Na 23 amu 23 g/mol 6.022 x 1023 atoms O 16 amu 16 g/mol 6.022 x 1023 atoms
- 7. Mole The mass in grams of one mole of substance called molar mass. Compound Molecular Mass /Formula Mass Molar Mass Avogadro’s Number CO2 44.0 amu 44.0 g/mol 6.022 x 1023 molecules Na2S 78.05 amu 78.05 g/mol 6.022 x 1023 formula unit
- 8. To calculate the number of moles of given element/compound, the formula is:
- 9. Sample Problem: 1.Gold (Au) is used in jewelry making. The atomic weight of gold is 197. Find the ff: ◦ a. number of moles ◦ b. number of atoms in 200 grams gold
- 10. Sample Problem: 2. Suppose you consume 500grams sugar (C12H22O11) in one week. How many moles of sugar did you consume? Calculate the number of molecules in 500grams sugar? Molar mass of sugar is 342 grams per mole.
- 13. Wellington Flour Mills Company Founded by Mr. Norberto Ty and Mrs. Salustiana Dee Ty since 1954 Flour has chemical formula of C4H8O4 Molar mass of 120g/mol
- 16. Convert Mass to the number of Particles
- 20. Concept Mapping 1. Analyze the concept map of each conversion factor 2. Write in the box the relationship in words 3. Write the relationship in units.
- 22. new unit original given concept map conversion factor
- 24. Title Lorem Ipsum 2017 Lorem ipsum dolor sit amet 2018 Lorem ipsum dolor sit amet 2019 Lorem ipsum dolor sit amet 2020 Lorem ipsum dolor sit amet
Editor's Notes
- However, since atom has such small masses, no usable scale can be devised to weigh them in calibrated instruments or units of atomic mass.
- However, since atom has such small masses, no usable scale can be devised to weigh them in calibrated instruments or units of atomic mass.
- One of the pioneers in the Philippines flour industry is the Wellington Flour Mills Company located at Barangay Pineda, Pasig Boulevard, Pasig City. Founded by Mr. Norberto Ty and Mrs. Salustiana Dee Ty since 1954.The Wellington Flour Mills has traditionally been known for producing high quality flour products. Flour is the most useful item in cooking. You can use it to make delicious cakes, bread, pastries and dessert. The chemical formula of flour is C4H8O4with the molar mass of 120g/mol. Let’s analyze the elemental composition of flour.