slide1
Download
Skip this Video
Download Presentation
Avogadro’s Number

Loading in 2 Seconds...

play fullscreen
1 / 28

Avogadro’s Number - PowerPoint PPT Presentation


  • 112 Views
  • Uploaded on

Avogadro’s Number. 6.02x10 23. mole = (mol) 602000000000000000000000. Mole. A mole is just a number like… Pair = 2 Trio = 3 Dozen = 12 Baker’s dozen = 13 Gross = 144 Score= 20 Century=100 Ream=500. How BIG is a mole?. There are ~ 6.6 billion people on Earth

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about 'Avogadro’s Number' - psyche


An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
slide3
mole = (mol) 602000000000000000000000Mole
  • A mole is just a number like…

Pair = 2 Trio = 3

Dozen = 12 Baker’s dozen = 13

Gross = 144 Score= 20

Century=100 Ream=500

how big is a mole
How BIG is a mole?

There are ~ 6.6 billion people on Earth

How many Earths would it take to equal the population

of 1 mole?

9.12 x 1013

slide5
If you spent $800 billion dollars a day how many years would it take to spend a MOLEion dollars?

2.06 x 109 years

slide6
If you had a mole of cats . . .

They would create a sphere

larger than

Earth!

slide8
If you had a mole of H2O could you swim in it?

NO! 

Water molecules are so small

that a mole of H2O = 18ml

slide9
In chemistry we don’t work with individual atoms or molecules because they are too small to be weighed or measured
  • We have to work with LOTS of atoms in order to measure them

THAT’s WHERE THE

MOLE COMES IN!

how small are atoms
How small are atoms?
  • There are more atoms in one gram of salt than grains of sand on all the beaches

of all the oceans in all

the world.

gram atomic mass
of the

in

Gram ATOMic Mass
  • mass is in grams of 1 mole of atoms of an element
  • In other words……

1 mol C atoms = 6.02 x 10 23 C atoms = 12g C

gram formula mass gram molecular mass molar mass
of the

in

Gram Formula MassGram Molecular Mass Molar Mass
  • mass in grams of 1 mole of a substance
  • In other words . . . Add it all up!

1 mole of NaCl = 58g = 6.02x1023 particles of NaCl

1 mole of H2O = 18g = 6.02x1023 molecules of H20

slide16
Now…..
  • Use the gram formula mass and the gram atomic mass to determine
    • how many moles or atoms of an element are found in some mass of a substance
    • how much mass that element contributes to the mass of the entire substance

Use factor label & follow the units!

stoich iometry of chemical formulas1
Stoichiometry of Chemical Formulas
  • If you have 1 molecule of (NH4)2SO4
    • How many atoms of N are there?
    • How many atoms of H?

SO…..

  • If you have 1 mole of of (NH4)2SO4
    • How many moles of N are there?
    • How many moles of H?
molar volume
Gases ONLY

@STP

Molar Volume
  • 1 mole of ANYgas

O2 (g)

NH3 (g)

He (g)

contains 6.02 x 1023 molecules and

occupies a volume of 22.4L

slide20
STP

standardtemperature & pressure

0oC or 273K

101.3kPa or 1 atm

remember
Remember . . .
  • Gases also have mass

1 mole of O2(g) = 32g

1 mole of NH3(g) = 17g

 we can calculate Density!

d m v
D = m/v
  • A sample of oxygen contains 3 moles of particles at STP what is its density?
  • 2 steps
    • Convert moles to mass AND volume
    • Calculate density
  • If mass or volume is given, use it and convert the other……. THEN calculate D!
slide23
Remember . . .

1 mole = 6.02x1023atoms or molecules =gfm = 22.4L (g)

stoich iometry of chemical equations
“it’s a simple matter

of weight ratios . . .”

Stoichiometry of Chemical Equations
  • The study of quantitative relationships that can be derived from chemical equations.
stoichiometry cookies
Stoichiometry cookies
  • If you look at chemical equations as recipes it may be easier to understand that
    • changing the amount of a reactant will change the amount of the product IN THE SAME RATIO!
examining molar relationships in balanced equations
Examining Molar Relationships in Balanced Equations

6CO2 + 12 H2O + 2804kJ  6O2 + C6H12O6 +6H20

Balanced equations

  • Law of conservation of mass / matter
    • ATOMS are not createdor destroyed during a chemical reaction, they are only rearranged to form new substances.
    • # atoms on reactant side = # atoms on product side
  • Law of conservation of E
    • E on the reactant side = E on the product side
ad