What’s in a mole
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The document provides instructions for conducting an experiment to measure the mass of paper clips using a balance and compute the number of paper clips in a handful based on the average mass. It asks students to record their results in a table and compare the computed number of paper clips to the actual counted number, explaining any differences. It then provides background information on moles as a unit of measurement in chemistry, defining it as 6.02 x 1023 particles and providing examples of converting between numbers of particles and moles for different substances using molar mass.
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Similar to What’s in a mole
Ib quan chemistry(mole concept)
1. The relative formula mass of calcium carbonate (CaCO3) is 100 g/mol.
2. One mole of calcium carbonate will react with 2 moles of hydrochloric acid (HCl).
3. Therefore, the mass of hydrochloric acid that will react with 1 mole (100 g) of calcium carbonate is 2 x 36.5 g = 73 g, since the molar mass of HCl is 36.5 g/mol.
MRS. RENEROSA G. CAMAY'S SIM
The document discusses the mole concept in chemistry. It provides guide cards explaining what a mole is, how to calculate molar mass, and how to convert between moles, mass, and number of particles. It includes activity cards with practice problems on these topics. The goal is to help students understand intricate topics in chemistry, like the mole, and enhance their critical thinking skills.
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 .
Chem m16 stoichiometry
This chemistry module discusses stoichiometry and the mole concept. It contains 4 lessons:
1) Defining a mole and the mole-particle relationship.
2) Exploring the mole-mass relationship through examples and activities.
3) Relating the mass of reactants and products in chemical equations using moles.
4) Calculating mass percent composition of elements in compounds.
The module aims to teach students how to use moles to relate mass, number of particles, and chemical equations.
Moles
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.
Stoichiometry
A mole is a specific amount of 6x1023 particles of an element or molecule. Moles allow conversions between mass, number of particles, volume, and concentration. Balanced chemical equations provide mole ratios to solve multi-step stoichiometry problems involving excess reactants or product yields. Empirical formulas give the simplest whole number ratio of elements in a molecule.
07 moles
This document provides information and examples about performing calculations involving moles, concentrations, and volumetric analysis (titrations). It explains the relationships between moles, volume, and molarity in solutions. It also outlines the basic steps for solving titration problems, including writing balanced equations, determining mole ratios, converting between masses and moles, and using the appropriate formula to calculate the unknown value. Several examples are worked through to demonstrate the method. The document concludes with practice problems for the reader to work through.
Introduction to stocihiometry milestone
Stoichiometry is the calculation of quantities in balanced chemical reactions. It allows chemists to determine the amounts of reactants needed and products expected based on balanced equations, similar to recipes. The document reviews key stoichiometry concepts like moles, molar mass, and mole ratios that allow conversions between masses, moles of substances, and atoms. It provides examples of using mole ratios from balanced equations to solve stoichiometry problems involving amounts in grams, moles, or particles.
Stoichiometry1.ppt
The document provides information about the mole concept in chemistry. Some key points:
- A mole is equal to Avogadro's number of particles of a substance, which is 6.022x1023 particles.
- One mole of any substance has a mass in grams equal to its formula mass or molar mass.
- Stoichiometry problems use the mole concept to calculate amounts of substances in chemical reactions based on molar ratios and molar masses.
- Examples are provided for calculating moles, masses, empirical formulas, and volumes of gases from given amounts of reactants.
Chapter 10 notes
The document provides notes on moles, molar mass, empirical formulas, and molecular formulas, including how to convert between units like grams, moles, particles, and volume using molar mass and stoichiometry. It defines key terms like moles, molar mass, empirical formula, and molecular formula. Examples are provided for calculating molar mass, moles, empirical formulas, and molecular formulas.
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.
mole.ppt
It would take approximately 19 million years to spend a mole of $1 coins if they were being spent at a rate of 1 billion per second.
A mole is equal to 6.022x10^23 items or entities. If 1 billion $1 coins were being spent per second, and there are 6.022x10^23 coins in a mole, it would take 6.022x10^14 seconds to spend a mole of coins. This equals approximately 19 million years.
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.
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.
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.
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 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.
Chemistry M2 Mole concept
The document discusses methods for converting between moles, mass, and number of particles for chemical substances:
1) Equations are provided to convert between moles and mass using molar mass, as well as to find the number of particles from moles using Avogadro's number.
2) Worked examples demonstrate using the formulas to calculate moles from mass and vice versa, as well as converting moles to number of atoms or molecules.
3) Determining empirical and molecular formulas from percentage composition by mass is explained. The empirical formula is used to calculate the molecular formula by considering the mass and moles of the empirical formula unit.
Lecture 10.1- The Mole
The document discusses the mole, which is used to measure the quantity of particles in chemical reactions. A mole is defined as 6.02 x 1023 particles and represents atoms, molecules, or formula units that are involved in a balanced chemical equation. The mass of one mole of an element or compound, known as its molar mass, is equal numerically to the atomic/formula mass and given in grams. The mole allows chemists to quantitatively relate the masses of reactants and products in chemical reactions.
Similar to What’s in a mole (20)
This activity is designed to introduce a convenient unit used by.docx
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What’s in a mole
- 7. A PAIR = 2 A DOZEN = 2 A BOX = 100 OR 30 0R 50 A PINCH = ? A BOWL = ? A SACK = ?
- 8. 1. Measure and record the mass of 25 pcs. Paper clip using the platform balance. Divide the mass obtained by 25 to find the average mass of one Paper clip. Perform 3 trials. Record your answers on a table. 2. Get a handful of paper clips and measure their mass. Compute for the number of paper clips using your data from step 1. Be sure to do it through computation and not by counting. 3. This time, count the number of paper clips in the handful paper clips in step 2. 4. Repeat steps 2 and 3 by getting different handful of paper clips. Record your answers on a table.
- 9. Is the number of paper clips in step 2 the same as the number of paper clips in step 3? Why do/don’t you think so?
- 10. The number of particles in one mole of a substance
- 11. A very large number equal to 6.02 X 1023
- 12. So, a mole (mol) of a substance is a representative particles of that substance.
- 13. • A unit of measurement in the International System of Units (SI) for amount of substance. • It is defined as the amount of a substance that contains as many elementary entities, e.g., atoms, molecules, ions, formula units, as there are 12 grams of carbon-12 atom.
- 14. 1 mole of a substance =6.02 X 1023 particles
- 15. 1 mole of C-12 atom =6.02 x 1023 particles = 12g 1 mole of H2O molecule = 6.02 x 1023 particles = 18g 1 mole of NH4+ ion = 6.02 x 1023 particles = 18g 1 mole of CaO formula units = 6.02 x 1023 particles = 36g
- 16. The mass of an element or compound depends on the mass of the particles. Therefore one mole of Carbon has a mass dependent on its atomic mass – MOLAR MASS MOLAR MASS = the mass in grams that is numerically equal to the atomic mass. The unit of molar mass is grams/mole (g/mol).
- 17. 1. How many molecules are there in 4.0 moles of CO2? To answer this, you have to consider that 1 mole of CO2 is equal to 6.02 x 1023 particles of CO2. Thus, using dimensional analysis approach, you will be able to convert the number of mole to its equivalent amount in the number of particles. 4.0 moles of CO2 = 6.02 x 1023 particles = 2.41 x 1024 molecules of CO2 1 mole of CO2
- 18. 2. How many moles of H2O are there in 1.79 x 10 24 molecules of H2O? To answer this, you have to consider that 1 mole of H2O is equal to 6.02 x 1023 particles of H2O Thus, using dimensional analysis approach, you will be able to convert the number of molecules to its equivalent amount in the number of moles. 1.79 x 10 24 molecules of H2O= 1 mole of H2O = 2.97 moles of H2O 6.02 x 1023 molecules of H2O
- 19. 1.How many mongo seeds are equal to 3.50 moles of Mongo seeds 2. How many moles of rice grains are equal to 1.807 x 10 24 grains of rice?
- 20. 1.How many bananas are equal to 7.50 moles of Bananas 2. How many moles of tomatoes are in 3.01 x 10 23 pieces of tomatoes?
- 21. “ Even a small act of kindness will make a great difference in people’s lives…” THANK YOU!