### Mole Conversions ppt - Coal City Unit District #1

```Round all masses to the 10ths place
 Step
One: two atoms of iron and three of oxygen
 Step
Two: Fe = 55.8 amu and O = 16.0 amu
 Step
Three: (2 x 55.8) + (3 x 16.0)
 Step
Four: 111.6 + 48.0 = 159.6 amu (grams) for
one mole
 Step
One: one atom of potassium, one of chlorine,
and four of oxygen.
 Step
Two: K = 39.1 amu, Cl = 35.5 amu, O = 16.0
amu
 Step
 Step
Three: (1 x 39.1) + (1 x 35.5) + (4 x 16.0)
Four: 39.1 + 35.5 + 64.0 = 138.6 amu (grams)
for one mole
 Step
One: two atoms of nitrogen, eight of hydrogen
and one of sulfur
 Step
Two: N = 14.0 amu, H = 1.0 amu, S = 32.1 amu
 Step
Three: (2 x 14.0) + (8 x 1.0) + (1 x 32.1)
 Step
Four: 28 + 8.0 + 32.1 = 68.1 amu (grams) for
one mole
 Calculate
 Al(1
the molar mass of Al(NO3)3
x 27.0) + N(3 x 14.0) + O(9 x 16.0) =
 213.0
amu (grams) is the mass of one mole of
aluminum nitrate.
 1.
AlCl3
 2. Ba(SCN)2
 3. LiH
 4. Ba(BrO3)2
 5. AlBr3
 6. HCl
 1.
 2.
 3.
 4.
 5.
 6.
133.5 g/mol
253.5 g/mol
7.9 g/mol
393.1 g/mol
266.7 g/mol
36.5 g/mol
Round all final answers to 3 sig figs
 KMnO4 = 158.0
g / mole of KMnO4
 Now
let’s solve it
 25.0
g x 1 mole = 0.158191804 moles
158.0 g
 0.158
moles
 H2O2
= 34.0 g / mole
 Now,
let’s solve it
 17.0
g x 1 mol H2O2 = 0.5 moles
34.0 g
 0.500
moles
 Calculate
the moles present in:
 1) 2.00 grams of H2O
 2) 75.57 grams of KBr
 3) 100. grams of KClO4
 4) 8.76 grams of NaOH
 5) 0.750 grams of Na2CO3
 Remember
to round answers to 3 sig figs
 1)
 2)
 3)
 4)
 5)
0.111 moles
0.635 moles
0.722 moles
0.219 moles
0.00708 moles
Round all answers to 3 sig figs
 H2O2
molar mass = 34.0 grams/mole
 0.700
moles x 34.0 grams = 23.8 g
1 mole
 23.8 grams
 KClO3
 2.50
molecular mass = 122.6 g/mole
moles x 122.6 g = 306.5 grams
1 mole
 307 grams
 Calculate
 1)
 2)
 3)
 4)
 5)
the grams present in:
0.200 moles of H2S
0.100 moles of KI
1.500 moles of KClO
0.750 moles of NaOH
3.40 x 10-5 moles of Na2CO3
 Remember
to round answer to 3 sig figs
 1)
 2)
 3)
 4)
 5)
6.82 grams
16.6 grams
136 grams
30.0 grams
0.00360 grams
6.02 x 1023 particles = 1 mole
Particles can mean atoms or molecules
 One
mole of donuts contains 6.02 x 1023
donuts
 One
mole of H2O contains 6.02 x 1023
molecules
 One
mole of nails contains 6.02 x 1023 nails
 One
mole of Fe contains 6.02 x 1023 atoms
 One
mole of dogs contains 6.02 x 1023 dogs
 One
mole of electrons contains 6.02 x 1023
electrons
 One
mole of Chemistry students contains
6.02 x 1023 poor, suffering (I mean happy,
joyful) high school students
 0.450
=
mole Fe x 6.02 x 1023 atoms
1 mole
2.709x1023 atoms
 Final,
 0.200
=
mole x 6.02 x 1023 atoms
1 mole
1.204x1023 atoms
 Final,
 1)
Calculate the number of molecules in
1.058 mole of H2O
 2)
Calculate the number of atoms in 0.750
mole of Fe
 Remember
to round to 3 sig figs
 1)
6.37x1023 molecules
 2)
4.52x1023 atoms
Grams to particles OR particles to grams
Grams to atoms OR atoms to grams
If MOLE is not stated, it’s a two step problem
ROUND ALL ANSWERS TO 3 SIG FIGS
 0.450
g x 1 mole Fe x 6.02x1023 atoms =
55.8 g
1 mole
 4.8548387x1021
 Final
atoms
 H2 O
molecular mass = 18.0 g
 0.200
g x 1 mole H2O x 6.02x1023 molecules
18.0 g
1 mole
 6.6888888889x1021
 Final
molecules
 1)
Calculate the number of molecules in
1.058 gram of H2O
 2)
Calculate the number of atoms in 0.750
gram of Fe
 Remember
to round answer to 3 sig figs
 1)
3.54x1022 molecules
 2)
8.10x1021 atoms
```