lecture 10.1- the mole
DESCRIPTION
Section 10.1 lecture for Honors & Prep ChemistryTRANSCRIPT
![Page 1: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/1.jpg)
QuickTime™ and a decompressor
are needed to see this picture.QuickTime™ and a
decompressorare needed to see this picture.
Lecture 10.1- The Mole
We often measure the amount of something by count, by mass, or by volume.
QuickTime™ and a decompressor
are needed to see this picture.
![Page 2: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/2.jpg)
In chemical reactions, atoms, molecules & salts react in specific ratios.
A chemist must be able to count molecules in order to run a reaction without having any leftover reactants.
QuickTime™ and a decompressor
are needed to see this picture.
![Page 3: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/3.jpg)
Atoms and molecules are very small.We need a very large number of atoms in order for a sample to be seen and worked with in a lab.The mole is a very big number!
![Page 4: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/4.jpg)
The mole is the SI unit used to measure quantity.
A mole is 6.02 x 1023 particles602 000 000 000 000 000 000 000
6.02 x 1023 is Avogadro’s number
![Page 5: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/5.jpg)
A mole is 6.02 x 1023 representative particles
![Page 6: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/6.jpg)
Representative particles
The representative particle for covalent compounds is the molecule.
For most elements the r.p. is the atom,
but for diatomic elements it is the molecule
H2 N2 O2 F2 Cl2 Br2 I2
For salts it is the formula unit.
![Page 7: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/7.jpg)
The official definition of one mole is the number of atoms in 12 grams of carbon-12.
![Page 8: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/8.jpg)
The mole is a very big number!
• A mole of inches is 1,616,434 light years, or across our galaxy and back 8 times!
• 6.02 X 1023 Donut Holes: Would cover the earth and be 5 miles (8 km) deep.
• 6.02 X 1023 Pennies: Would make at least 7 stacks that would reach the moon.
• 6.02 X 1023 Grains of Sand: Would be more than all of the sand on Miami Beach.
• 6.02 X 1023 Blood Cells: Would be more than the total number of blood cells found in every human on earth.
• 1 Liter bottle of Water contains 55.5 moles H2O
• 5 Pound Bag of Sugar contains 6.6 moles of C12H22O11
![Page 9: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/9.jpg)
Converting moles to number of particles
How many atoms are in 3.5 moles of Cu?
3.5 moles Cu
6.02x1023 atoms 1 mole Cu
X = 2.1 x 1024 atoms
6.02 x 3.5 ≈ 21 21 x 1023 = 2.1 x 1024
![Page 10: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/10.jpg)
Converting number of particles to moles
We have 3.0 x 1025 molecules of water.
How many moles?3.0 x 1025 molecules
X _____1 mole______ 6.02 x 1023 molecules
≈ 50 moles of water
![Page 11: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/11.jpg)
0.5 x 10(25-23) = 0.5 x 102
= 5 x 101
6.02 1023
3.0 x 1025
6.02 x 1023
≈ 50 moles of water
3.0 x 1025
![Page 12: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/12.jpg)
Find out how Avogadro’s number is based on the relationship between the amu and the gram.
QuickTime™ and aSorenson Video 3 decompressorare needed to see this picture.
![Page 13: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/13.jpg)
The atomic mass is the mass of a single atom of a specific element (with units of amu).
The mass of one mole of a specific element (measured in grams) is known as its molar mass.The numerical value of both are equal, only the units change.
![Page 14: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/14.jpg)
One atom of calcium has an atomic mass of 40.078amu.
One mole of calcium has a molar mass of 40.078g.
![Page 15: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/15.jpg)
Lead 207.2amu per atom
207.2g per mole
![Page 16: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/16.jpg)
Using the mole allows us to “count” the number of particles in a sample by mass.
QuickTime™ and aYUV420 codec decompressor
are needed to see this picture.
![Page 17: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/17.jpg)
The molar mass of each element is given on the periodic table.
The Mass of a Mole of an Element
![Page 18: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/18.jpg)
The Mass of a Mole of an Element
•One molar mass of carbon, sulfur, mercury, and iron are shown.
![Page 19: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/19.jpg)
To calculate the molar mass of a compound, add the masses of the elements in the compound.
The Mass of a Mole of a Compound
![Page 20: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/20.jpg)
• Substitute the unit grams for atomic mass units. Thus 1 mol of SO3 has a mass of 80.1 g.
SO3 contains 1 S and 3 O 1 x 32.1(mass of S) = 32.1 g 3 x 16.0(mass of O) = 48.0g
32.1 + 48 = 80.1g/mol of SO3
![Page 21: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/21.jpg)
• Molar Masses of Glucose, Water, and Paradichlorobenzene
The Mass of a Mole of a Compound
![Page 22: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/22.jpg)
1 mole is 6.02 x 1023 of anything
![Page 23: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/23.jpg)
10.4
![Page 24: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/24.jpg)
![Page 25: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/25.jpg)
![Page 26: Lecture 10.1- The Mole](https://reader033.vdocument.in/reader033/viewer/2022052410/555cffbcd8b42a08668b538d/html5/thumbnails/26.jpg)
Molar Mass
Element- molar mass is on periodic table
Compound- Add the mass for each element in the compound.