Chapter 1-2 Mole concept
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This document discusses moles, atoms, molecules, and conversions between moles, mass, and number of particles. It defines a mole as the amount of a substance with the same number of particles as 12 grams of carbon-12. It states that one mole contains 6.022 x 10^23 particles, known as Avogadro's number. The mass of one mole of a substance is equal to its atomic or molecular mass. Examples are given of converting between moles and mass or number of particles.
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The mole concept
This document discusses moles, molar mass, and Avogadro's number. It explains that a mole is the amount of a substance that contains 6.022x1023 particles, known as Avogadro's number. It also defines molar mass as the mass in grams of one mole of a substance. The document provides examples of calculating molar mass from atomic masses and using molar mass to determine the number of moles or particles in a given mass of a substance.
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A mole is the standard unit used to measure very large quantities of small particles like atoms and molecules. It represents 6.02 x 1023 particles, which is an immense number that is difficult to comprehend. The molar mass of an element or compound is the mass in grams of one mole of that substance. To find molar mass, one does an atom inventory of the substance and multiplies the number of each type of atom by its atomic mass on the periodic table, then sums the results.
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The document discusses atomic and molecular masses, moles, molar masses, and calculating empirical and molecular formulas. It provides examples of calculating moles from masses and vice versa using molar masses. It also discusses calculating percentage compositions and determining molecular formulas from empirical formulas using molar masses.
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The document discusses the relationship between the number of moles, mass, and molar mass of substances. It defines molar mass as the mass of one mole of a substance in grams. Molar mass can be found on the periodic table for elements and is calculated by adding the molar masses of the constituent atoms for compounds. The document provides examples of calculating molar masses for common substances like water, sodium chloride, and aluminum and relates molar mass to Avogadro's constant of 6.022 x 10^23 particles per mole.
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The document provides an introduction to stoichiometry including the four types of stoichiometry problems: (1) given and unknown amounts in moles, (2) given amount in moles and unknown in grams, (3) given amount in grams and unknown in moles, and (4) given and unknown amounts in grams. It then works through example problems of each type, calculating amounts of products or reactants using molar ratios derived from balanced chemical equations.
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The document discusses the mole, which relates the number of particles in a substance to its mass in grams. It defines one mole as 6.02 x 10^23 particles, known as Avogadro's number. It provides examples of calculating moles, mass, and number of particles using molar mass and unit conversion with moles. Key relationships discussed are mass=moles×molar mass and number of particles=moles×Avogadro's number.
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This document discusses moles, molar mass, and Avogadro's number. It explains that a mole is the amount of a substance that contains 6.022x1023 particles, known as Avogadro's number. It also defines molar mass as the mass in grams of one mole of a substance. The document provides examples of calculating molar mass from atomic masses and using molar mass to determine the number of moles or particles in a given mass of a substance.
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A mole is the standard unit used to measure very large quantities of small particles like atoms and molecules. It represents 6.02 x 1023 particles, which is an immense number that is difficult to comprehend. The molar mass of an element or compound is the mass in grams of one mole of that substance. To find molar mass, one does an atom inventory of the substance and multiplies the number of each type of atom by its atomic mass on the periodic table, then sums the results.
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Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
INTRODUCTION
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Every topic of this chapter is well written concisely and visuals will help you in understanding and imagining the practicality of all the topics.
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- The mole can be used to convert between the number of particles/formula units and the mass of a substance using molar mass and the definition of 1 mole.
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The purpose of the study was to determine the students’ error in learning mole concept A total of 120
Senior Secondary 2 chemistry students randomly selected from two private schools in Zaria with a mean age of
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diagnostic test (MDT) were used as the instruments for the study . Diagnostic interview and semi-structured
questionnaire were also used to identify at which level students’ errors occur in solving problems and the
perception of students towards mole concept was that success can be achieved in problem solving with a good
grasp of the subject and an above average mathematical ability. The type of error analyzed were based on the
modified Newman Error Hierarchy Model that includes reading type error, comprehension, transformation,
process skill, and encoding error. Data was analyzed using mean, percentage, frequency, Duncan’s (MultipleRange)
and Wilcoxon test at P< 0.05. The study found out among others that the error most students make
involving transformation and process skill in solving problems in mole concept was significant (P<0.05) .There
was no error found in reading. The number of students who made encoding error and carelessness was small.
The students’ error in solving problems in mole concept was due to their weaknesses in stoichiometry and basic
arithmetical operations. The need for an appropriate and friendly pedagogical approach in the learning of mole
concept was proposed and recommendations were made based on findings
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The mole is a unit used in chemistry to measure the amount of a substance. It represents 6.02 x 1023 particles of anything. A mole is defined as the formula mass in grams of a substance. For example, the mass of one mole of chromium atoms is 51.9961 grams, which is equal to the mass of one atom in atomic mass units. The mole is a convenient unit for chemists because it allows them to relate the number of particles, formula mass, and molar mass of substances.
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Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
I have expertise in making educational and other PPTs. Email me for more PPTs at a very reasonable price that perfectly fits in your budget.
Email: parmarshivam105@gmail.com
Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
INTRODUCTION
MORE ABOUT MOLE
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MORE ABOUT MOLE CONCEPT
RELATIONSHIP BETWEEN MOLE, AVOGADRO NUMBER, AND MASS
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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 discusses the mole concept in chemistry. Some key points:
- A mole is the amount of substance containing Avogadro's number (6.022x1023) of elementary entities like atoms, molecules, formula units.
- One mole of any substance has a mass in grams equal to its formula/molar mass. For example, 1 mole of iron (Fe) has a mass of 55.85 g.
- The mole can be used to convert between the number of particles/formula units and the mass of a substance using molar mass and the definition of 1 mole.
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Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
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17 constituted the sample size for the study. The Chemistry achievement tests (CAT) and Mole concept
diagnostic test (MDT) were used as the instruments for the study . Diagnostic interview and semi-structured
questionnaire were also used to identify at which level students’ errors occur in solving problems and the
perception of students towards mole concept was that success can be achieved in problem solving with a good
grasp of the subject and an above average mathematical ability. The type of error analyzed were based on the
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process skill, and encoding error. Data was analyzed using mean, percentage, frequency, Duncan’s (MultipleRange)
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The document discusses key concepts in chemistry including atoms, molecules, ions, and moles. It introduces important historical figures like Antoine Lavoisier, John Dalton, and Amedeo Avogadro. It defines atoms as the smallest particles that make up elements and participate in chemical reactions. Molecules are groups of atoms bonded together. Ions are atoms or groups of atoms with a positive or negative charge. The mole concept relates the mass of a substance to its number of particles or molecules.
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The mole
The document defines a mole as a unit of measurement used in chemistry to represent very small numbers of particles. A mole is equal to 6.022 x 1023 representative particles, whether atoms, molecules, ions or other units. Examples show that 1 mole of an element equals its atomic mass in grams, and 1 mole of a compound equals its molar mass in grams. Common mole conversions involve changing between mass, moles, number of particles, and volume of gases.
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.
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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.
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The document discusses the mole, Avogadro's number, molar mass, and how they relate to converting between the number of particles, moles, and mass in chemical substances. The mole is defined as 6.022x10^23 particles of a substance, known as Avogadro's number. Molar mass is the mass in grams of one mole of a pure substance and can be calculated from atomic or molecular masses on the periodic table. Conversions between moles, number of particles, and mass use molar mass and Avogadro's number.
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This document provides an overview of moles, molar mass, and stoichiometry. It defines a mole as 6.02x1023 particles of an element or compound. Avogadro's number is equal to this quantity of particles. Molecular mass is the mass of one molecule in atomic mass units (amu) while molar mass is the mass of one mole of a substance in grams. Examples are given for calculating molecular and molar mass. The document then discusses balancing chemical equations and using molar ratios from balanced equations to solve stoichiometry problems involving moles, grams, and particles of reactants and products.
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The document provides information on stoichiometry, including:
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This chapter discusses the mole as a unit for measuring amounts of substances. It defines key terms like the mole, Avogadro's number, molar mass, and representative particles. It explains how to use molar mass to convert between mass and moles of a substance. The chapter also covers calculations involving chemical formulas, percent composition, and determining empirical and molecular formulas from experimental data.
Moles
1. A mole is a unit used to quantify an amount of substance and refers to 6.022x10^23 elementary entities, whether atoms, molecules, ions or other particles.
2. The mass of one mole of a substance can be calculated from its relative atomic/molecular mass. For example, one mole of carbon has a mass of 12g while one mole of oxygen has a mass of 32g.
3. Moles allow for stoichiometric calculations to determine amounts of reactants and products in chemical reactions and for calculating molar concentrations in solutions.
Moles
1. A mole is a unit used to quantify an amount of substance and refers to 6.022x10^23 elementary entities, whether atoms, molecules, ions or other particles.
2. The mass of one mole of a substance can be calculated from its relative atomic/molecular mass. For example, one mole of carbon has a mass of 12g while one mole of oxygen has a mass of 32g.
3. Moles allow for stoichiometric calculations to determine amounts of reactants and products in chemical reactions and for calculating molar concentrations in solutions.
c4e237864d12cdb0be66e0e86247e4cben4.pptx
Mole concept it's explanation and calculations on mole concept including concentration.
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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
Chemistry 2 yousef berbar
This document discusses concepts related to moles, molar mass, and stoichiometry. It defines key terms like mole, molar mass, and Avogadro's number. It explains how to calculate atomic mass using isotope ratios and explains that molar, molecular, and atomic mass have the same magnitude but different units. Examples are given for calculating molar mass of compounds like CO2 and H2O. Methods for solving stoichiometry problems using mole ratios and densities are demonstrated. Four sample problems and their solutions are presented to illustrate these concepts.
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.
CALCULATION OF MOLAR SOLUTION.pptx
The document describes key concepts related to moles, molar mass, concentration, and molar volume. It defines a mole as a specific number of entities, such as atoms or molecules, and describes how to use molar mass to convert between moles and mass. It also explains how to calculate molarity of solutions and how to dilute solutions. Finally, it provides the definition of molar volume as the volume occupied by one mole of a gas under standard temperature and pressure and shows examples of calculations related to moles and molar volume.
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This document discusses key concepts related to stoichiometry including:
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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
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.
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).
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Chapter 1-2 Mole concept
- 2. Small Large in number Difficult to count Difficult to weigh ATOM
- 3. One mole of substance is the amount of substance that has the same number of par<cles as there are in 12g of Carbon-‐12. Mole
- 4. Like :! ! 1 dozen = 12! 1 pair = 2! ! Similarly:! 1 mole = 6.022 x 10 23 of anything! !
- 5. What is Avogadro number? Avogadro number = 6.022 x 10 23!
- 6. What is Atomic Mass in terms of moles? Mass of 1 mole of atoms = Atomic mass!
- 7. What is Molecular mass in terms of moles? Mass of 1 mole of molecules = molecular mass!
- 8. Conversions-‐ Mole and Mass
- 9. Conversions-‐ Mole and Mass How many moles of Carbon are present in 24 grams of Carbon?!
- 10. Conversions-‐ Mole and Number of atoms/molecules
- 11. Conversions-‐ Mole and Number of atoms/molecules How many atoms of Carbon are present in 2 moles of Carbon?!