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This lecture outline from chem 1075 covers the concept of the mole as a unit of measure in chemistry. Topics include the comparison of dozens and moles, the definition and properties of the mole, mole calculations, and the relationship between atomic mass and molar mass. Slides include examples and practice problems.
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Chem 1075 Chapter 9 The Mole Concept Lecture Outline Slide 2 Dozen compared to Mole We use “dozen” to _________________________________; We know 1 dozen = _______________ We use “mole” to ___________________________________________________________________ Slide 3 The Mole The mole (mol) is a unit of measure for the ________________________________________in a chemical substance. A ____________ is _____________________________________(abbreviated “N”) of particles or _______________________________particles. 1 mol = Avogadro’s number = ___________________________ particles. We can use the __________relationship to convert between the number of __________________ and the _________________ of a substance. Slide 4 How Big is a Mole? The volume occupied by 1 mole of _________________________would be about the size of the _______________________. One mole of Olympic shotput balls has about the same _______________as the _________________. Slide 5 Mole Calculations I Use Avogadro’s number to convert between _________________________ and _______________: __________________________particles = _________ mole
Slide 6 Mole Calculations I How many sodium atoms are in 0.120 mol Na?
Slide 7 Mole Calculations I How many moles of potassium are in 1.25 x 10^21 atoms K?
Slide 8 Practice
Slide 9 Atomic Mass vs. Molar Mass
Slide 18 Pressure and Units Pressure is defined as the ratio of ____________________per unit _________________ (i.e. psi)
Slide 19 Molar Volume of Gases ______mole gas = _____________________molecules gas = ___________L gas
Slide 20 Gas Density
Slide 21 Calculating Gas Density
Slide 22 Molar Mass of a Gas
Slide 23 Mole Unit Factors
Slide 25 Mole-Volume Calculation A sample of methane, CH 4 , occupies 4.50 L at STP. How many moles of methane are present?
Slide 26 Mass-Volume Calculation What is the mass of 3.36L of ozone gas, O 3 , at STP?
Slide 27 Molecule-Volume Calculation How many molecules of hydrogen gas, H 2 , occupy 0.500L at STP?
The ____________________ of radium is ____________ g/mol and the ______________________ of oxygen is ________________ g/mol. (Comes from periodic table)
The ratio of elements in benzene is C_________H__________. Divide by the _________________________number to get the formula:
Slide 38 Molecular Formulas The _____________________ formula for benzene is CH. This represents the __________________ ratio of C to H atoms of benzene. The actual molecular formula is some ___________________ of the empirical formula, ___________ Benzene has a molar mass of 78 g/mol. Find n to find the molecular formula.
Slide 39 Overview of Calculations