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Molecules OR atoms
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3 mol Ne
1
1
6.02x1023 atoms
1 mol
!*
6.02x1023 particles
1 mol
1 mol
6.02x1023 particles
%
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Molecules?
’s
Nu
m
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Av
og
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ro
6.02x1023 particles
1 mol
Atoms
be
r
PARTICLES
1 mol
6.02x1023 particles
MOLES
%
6 mol O2
1
%
)$
6.02x1023 molecules O2
1 mol O2
8.02x1020 molec. I2
1
<
5
2 atoms O
1 molec. O2
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1 mol I2
6.02x1023 molecules I2
@
7.22x1024 atoms O
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1.33x10-3 mol I2
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mol
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g
MOLES
%
14 g LiOH
1
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1 mol LiOH
23.95 g LiOH
%
15 g N2
1
@
0.58 mol LiOH
.? $9 @
1 mol N2
28.02 g N2
0.54 mol N2
%
4 mol H2O2
1
%
56 mol CaCO3
1
$
2
34.016 g H2O2
1 mol H2O2
$
100.09 g CaCO3
1 mol CaCO3
@
136.06 g H2O2
?5
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5605.04 g CaCO3
+
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3.
PARTICLES
Avogadro’s
Number
MOLES
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250 g C12H22O11
1
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1 mol C12H22O11
342.3 g C12H22O11
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1 mol C12H22O11
4.4x1023 molec. C12H22O11
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1
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6.02x1023 molec. CH4
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24
16.016 g CH4
1 mol CH4
106.42 g CH4
6
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MASS
PARTICLES
Molar
Mass
Avogadro’s
Number
MOLES
Molar Volume
(22.4 L/mol)
VOLUME
of gases at STP
6
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4
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0
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1.0-L CO2
1
%
:
6.02 x 1023 molec CO2
1 mol CO2
1 mol CO2
22.4 L CO2
6
%
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B(
@
$
0.82 mol O2
1
2.7 x 1022 molec. CO2
22.4 L O2
1 mol O2
)$ $ * A
18 L O2
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total mass of compound
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B
Number of
particles
A
Moles of
substance
E
D
C
Mass of
substance
F
Volume of gas
(STP)
a)
Use N as a unit factor: multiply by 1 mol/6.02x1023
b)
Use N as a unit factor: multiply by 6.02x1023/1 mol
c)
Use molar mass as a unit factor: multiply by 1 mol/#g
d)
Use molar mass as a unit factor: multiply by #g/1 mol
e)
Use molar volume as a unit factor: multiply by 1 mol/22.4L
f)
Use molar volume as a unit factor: multiply by 22.4L/1 mol