the mole road map chemistry unit 6: chemical quantities lecture 6.4
TRANSCRIPT
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The Mole Road Map
Chemistry
Unit 6: Chemical Quantities
Lecture 6.4
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Objectives
• Convert a quantity of a chemical between moles, mass (g), particles, and volume.
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ALL About the Mole…
• We have now looked at the mole in terms of mass (g), particles, and volume.
• HOWEVER…in order to do these conversions, one of our units had to be the mole.
• What do you do, if you are asked to convert between two units and neither one is mole?
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Everything Goes Through The Mole!
• To convert from one unit to another, you must use the mole as an intermediate step.
• In other words…you might need a “two-step” conversion problem.
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What is a “Two-Step” Conversion Problem?
• Two conversion factors– One to convert from given unit to moles– One to convert from moles to wanted unit
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Mole Road Map
Mass
Representative Particles
Mole
22.4 L
1 mol
1 m
ol
22.4
L
1 mol
6.02x10 23 particles
Molar mass
1 mol
1 m
ol
Mola
r mas
s
6.02x1023 particles
1 mol
(grams) (atoms, molecules, or formula units)
Volume
of gas
(STP)
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Here’s An Example
Calculate the number of molecules in 60.0 g NO2.
Given: 60.0 g NO2
1st Equality: Molar Mass Equality
molar mass NO2 : 46.01 g46.01 g = 1 mol
2nd Equality: Definition of Mole Equality1 mol = 6.02 x 1023 molecules
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So here’s the equation:
60.0 g NO2 x 1 mol x 6.02 x 1023 molecules =
1 46.01 g NO2 1 mol
7.85 x 1023 molecules NO2
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Another Example
Calculate the volume, in liters, of 3.24 x 1022 molecules of Cl2 (STP).
1.21 L Cl2
3.24 x 1022 molecules Cl2 x 1 mol x 22.4 L Cl2 = 1 6.022 x 1023 molecules 1 mol
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What Now?
• You will NOT be allowed to use your “Road Map” on the test, so you need to practice enough that you no longer rely on it to help you through solving these problems.