Quantities in Chemical Reactions

Slides:



Advertisements
Similar presentations
Unit 7: Chemical Quantities
Advertisements

Stoichiometry: Mathematics of Chemical Formulas and Equations.
Section 10.1 Measuring Matter
Quantities in Chemistry The Relationship Between Mole and Molar Mass.
 Definition: Avogadro's number is the number of particles found in one mole of a substance. It is the number of atoms in exactly 12 grams of carbon-12.
X Chemistry Unit 8 The Mole Problem Solving involving Chemical Compounds.
Ch. 3 Stoichiometry: Calculations with Chemical Formulas.
CHAPTER 10 Chemical Quantities. Before We Begin…  We need to review some scientific notation.scientific notation  Scientific notation is a way of writing.
Chemical Quantities Math in Chemistry. Measuring Matter measure the amount of something by one of three different methods— by count, by mass, and by volume.
Chapter 10 & 11 Chemical quantities and Chemical Reactions.
Lecture 5. Chapter 3. Chemical Equations:
Chemical Quantities and Moles
The Mole: A Measurement of Matter
Stoichiometry & the Mole. Dimensional Analysis Review How many seconds are in 5.0 hours?
The MOLE CH 11.
The Mole Chapter 11.
1 Chemistry 11 Chapter 4 - The MOLE. 2 Relative Atomic Mass Dalton, concerned with how much one element could combine with a given amount of element,
Counting Large Quantities Many chemical calculations require counting atoms and molecules Many chemical calculations require counting atoms and molecules.
Unit 2: Chemical Quantities SCH 4C. The Chemist’s Dozen  How many in a couple?  How many in a few?  How many in a dozen?  How many in a ream? 2 3.
Relating Mass to Numbers of Atoms The mole, Avogadro’s number, and molar mass provide the basis for relating masses in grams to moles.
Chapter 6: Moles, Molar Mass, Percent Composition and Formulas From moles to mass and to the moon!
Good Day! 11/23/2015 Starter: = 2! Please explain why this is true. Today we will be… First doing a very thourough cleaning of the lab equipment.
What is a Mole? To a chemist a mole is a counting unit for a substance. Abbreviated “mol”
Counting atoms. atomic number - # of protons in atom of an element identifies element tells also # of e- Au, K, C, V.
The Mole Concept... Quantities in Chemistry. Real Life Quantities How many shoes do you have? “I have 26 kg of shoes.” What’s wrong with this answer?
Quantities in Chemistry
Quantities in Chemistry The Mole and Molar Mass. Mole Review A Mole is a unit of measurement in chemistry. It represents 6.02 x of an entity. One.
Part 6 – Moles and Counting Atoms. Measuring Matter When we talk about “how much” of something we have we use three different ways of measuring: –Counting-
1. 2 Chemical Quantities or 3 How you measure how much? How you measure how much? n You can measure mass, n or volume, n or you can count pieces. n We.
The Mole. Atoms & molecules are extremely small The number of individual particles in even a small sample of something is very large Therefore, counting.
A. Measuring Matter 1. Statement Chemistry is a quantitative science. 2. What is one way to measure matter? One way to measure matter is to count how.
The Mole Pay Attention this is really important!.
The Mole Q: how long would it take to spend a mole of $1 coins if they were being spent at a rate of 1 billion per second?
Ch. 10- The Mole Why- Within the next 2 months we will be working with chemical quantities. Determining what a reaction will produce or how much we need.
Atomic Mass and The Mole Topic: AMU’s & Atomic Mass Objectives: Day 1 of 3 To learn how we define 1 amu (atomic mass unit) To learn how we derive atomic.
Chemical Quantities Key Question How can you convert among the count, mass, and volume of something? Knowing how the count, mass, and volume of.
The Mole iew_video.php?viewkey=accb 4798ce8a9857e3f6 1.
The Mole Chemistry – Chapter 11. Measuring Matter  What measurements do we use?  Pair  Dozen  Gross  Ream  Counting Particles  Atoms and molecules.
An Introduction…... Atomic Mass: Where can you find it? An atomic mass unit is defined as 1/12 the weight of the carbon-12 isotope. The old symbol was.
How to count things that are way too small to see, like… Atoms Ions Molecules Chapter 8 The Mole Concept.
THE MOLE... a unit of counting Quantities in Chemical Reactions.
The Mole. Dimensional Analysis Review How many seconds are in 5.2 hours?
7.4 The Mole A counting term states a specific number of items. The terms dozen, case, gross, and ream are used to count the number of items present.
Chapter 7 Chemical Quantities.
The Mole 6.02 X 1023 To play the movies and simulations included, view the presentation in Slide Show Mode.
Chapter 8 The Mole Concept
Chemical Sentences: Equations
Pay Attention this is really important!
The Mole Concept.
Ch. 10 Chemical Quantities
Chapter 10.1 The Mole: A Measurement of Matter
Chapter 11 The Mole.
Amounts in Chemistry Unit 2 Week 5 Tuesday.
Stoichiometry & the Mole
Chapter 9 “Chemical Quantities”
Avogadro’s number, the mole, molarity, molar mass
Introduction to Chemical Principles
Introduction to Chemical Principles
Avogadro’s Number: 1 mole = 6.02 x 1023 particles
Mole Conversions
Spark How can we count a million of something? Consider that counting 1 million baseballs at a rate of 1 baseball/second would take nearly 278 hours… Now.
Unit II – Quantities in Chemical Reactions
The Mole.
Chemical Quantities.
Chapter 2 Atoms and Elements
Created by C. Ippolito June 2007
Chapter 9 The Mole Concept by Christopher Hamaker
Chemical Calculations Lesson # 1
The Mole Chapter 7-1.
Presentation transcript:

Quantities in Chemical Reactions The Mole

Did you know? Count Lorenzo Romano Amedeo Carlo Avogadro di Quaregna e di Cerreto (1776-1856) was an Italian chemist, most noted for his contributions to the theory of molarity and molecular weight. He is commonly referred to as simply Amedeo Avogadro. In 1811, he proposed what is now known as Avogadro's law and Avogadro's number. He made a critical contribution (recognized only in 1860 after his death) which helped greatly with the measurement of atomic weights.

Counting in Chemistry Chemists are very interested in counting atoms, formula units and molecules of substances that participate in chemical reactions. However, it is not possible, or practical, to work with individual atoms in the lab, since they are too small and you wouldn't be able to see the results. It is necessary to work with large enough samples for you to see and weigh on a balance using units of grams. A pile of atoms big enough for you to see contains billions of atoms. It can be difficult to keep track of such large number in calculations, so chemists made up a new unit for it.

Avogadro's Number In 1811, Amedeo Avogadro published a hypothesis on the volume of gases, stating that equal volumes of gases, at the same temperature and pressure, contain the same number of molecules regardless of their chemical nature and physical properties. This number is so important that it has a name. It was later called Avogadro's number and has the symbol N. The value of Avogadro’s number was precisely determined to be 6.022 x 1023. This is a very large number (602 200 000 000 000 000 000 000) and has no unit.

The Mole How many of something is in a “dozen”? What is a “gross”? A pair? These are common groupings that correspond to specific values. The same thing occurs in chemistry. You can say there is an Avagadro’s number of atoms in a “mole” of atoms. Here is how the International Union of Pure and Applied Chemistry (IUPAC) defines the mole: “The mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon-12. When the mole is used, the elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles, or specified groups of such particles.” In other words, one mole contains as many entities as there are in 12 g of carbon-12 (or 0.012 kg). There are 6.022 x 1023 atoms in 12 g of carbon-12.

The Mole (con’t) The mole is abbreviated as “mol” Mol is the SI base unit for measuring how much of a substance is present. One mole of ANY specified entity contains 6.022 x 1023 of that entity: One mole of donuts contains 6.022 x 1023 donuts One mole of H2O contains 6.022 x 1023 molecules One mole of nails contains 6.022 x 1023 nails One mole of Fe contains 6.022 x 1023 atoms

Example 1 How many atoms are in 0.5 mol of sodium? 1 mole of anything corresponds to 6.02 x 1023 0.5 mol of sodium corresponds to x atoms of sodium There are 3.01 x 1023 atoms in 0.5 mol of sodium. This solution uses ratio reasoning. A similar answer could be obtained by multiplying the 0.5 mol of sodium by the unit factor [6.02 x 1023 atoms/mol].

Example 2

Check Your Understanding How many atoms are then in one molecule of Al(NO3)3? 3 5 11 13 How many atoms are there in 2 mol of iron? How many moles of tungsten correspond to 5.05 x 1020 atoms?