1. Chemistry 1 Notes # 3b Chapter 11 Section 1 THE MOLE & particle/mass calculations
Last updated November 18, 2018

2. MOLE
Moles- SI unit for the amount of a substance.

3. Practice with Dimensional Analysis
Convert 43,000 cm to miles
2.54 cm = 1 in.
12 in. = 1 ft.
3 ft. = 1 yd.
1,760 yds.= 1 mile
Convert 3.25 miles to meters

4. Measuring Matter What is a mole?
The Mole is an SI base unit for the amount of a substance.
6.02 x 1023 = number of representative particles in exactly 12 g of Carbon-12 = 1 mole

5. Whereas a dozen is known as 12 of something, a pair is always 2, and a gross is always This number never changes but what is counted does.
The same can be said about the mole

6. The mole represents 6.02x1023 of something.
This number is called Avogadro’s number
In chemistry the mole is used to measure how many atoms, particles or molecules something contains

7. Converting Moles to Particles and Particles to moles
Using the mole and knowing how many particles, atoms or molecules, converting from the mole to how many particles and back is simple
Problem: How many atoms are in 1.76 mol of Zn

8. Solution:

9. Particles to Moles How many mol are in 2.33x1027 particles of Carbon?
Actual answer 3870 mol C or 3.87 x 103 mol C

10. 11.2 Mass and the Mole
Molar mass  the mass in grams of one mole of any substance.
For example: The atomic mass of carbon is amu (atomic mass units) therefore the molar mass of carbong is grams
What is the molar mass of Potassium?

11. Molar mass of a Compound
To determine the molar mass of a compound simply add up the molar mass of each of the individual atoms that make up the compound.
Examples:
NaCl = g g = 58.44g/mol
H2O
2(1.01g) g= g/mol

12. Using Molar Mass Given moles convert to mass

13. Using Molar Mass Given Mass convert to moles

15. Mole Map