Download The Mole

Moles--Day 1: The Mole
Assignment: Chapter 11, problems 1-10
Reading: Chapter 11, pages 308-312
1.
List several names that are used to describe numbers.
2.
In chemical equations what do the coefficients represent?
12NaOH + Pb3(PO4)4  3Pb(OH)4 + 4Na3PO4
3.
Is it equally valid to say you have that many dozen of each compound? Why?
4.
Why isn’t it reasonable to deal with individual compounds or even dozens of compounds in
chemical reactions?
5.
What number do scientists use to evaluate chemical reactions on a realistic scale?
6.
How did scientists arrive at this value?
7.
List the mass of one mole (also known as Molar Mass) of the following elements.
Na
C
Ag
Au
Cu
F
8.
Why is this useful?
9.
Let’s back up a little. If you didn’t have the mole you would have to use the actual number of
atoms. Let’s see what number you would have to use instead of moles:
 6.02 x1023 atoms Ag 
3.0 mol Ag 

1 mol Ag


 6.02 x1023 atoms P 
2.3 mol P 

1 mol P



0.4 mol Au 

10.



Let’s say, for some reason, you knew the number of particles and you wanted to change that
number into moles. How would that work?


1 mol Ag
3.0 x1023 atoms Ag 

23
 6.02 x10 atoms Ag 


1 mol Ag
7.2 x1025 atoms Pb 

23
 6.02 x10 atoms Ag 

3.6 x1022 atoms K 

11.



For super duper extra points, how many oxygen atoms are in 3.2 moles of NaNO3?