Grams
Mole Map
Volume
of a
@ STP
Gas
22.4 L
mole
6.02 x 1023
molecules
# atoms
per
molecule
atoms
Atoms
(element)
Factor Label – It’s back…..
How many moles are in 45.7 g of NO2?
= 14.01 g +the
2(16.00
g) = 46.01–g Can I
1.Molar
Askmass
yourself
question
5.6.
Cancel
conversion
out
units
factor
and
calculate
that
will
using
allow
you
4.
2.Use
3.
Start
Calculate
Form
YES
with
–conversion
molar
Molar
your
mass
“given”
Mass
factors.
has
ofgrams
afrom
NO
unit
.
the
of
convert
directly
from
to
2
to
“cancel”
significant
out
digits.
grams
and give you moles.
original
problem.
grams/mole
moles?
7
8
1 mole
46.01Molar
g mass =
14.01 g + 2(16.00 g) = 46.01 g
N
O
46.01
g 15.9994
1 mole
14.00674
45.7 g NO2 x 1 mole = 0.993 mole NO2
46.01 g NO2
1
Factor Label – It’s back…..
How many atoms are in 10.0 moles of Iron (Fe)?
Use
that
allow
you
6.
Cancel
outyour
units
and
calculate
using
1. Start
Ask conversion
yourself
the“given”
question
–will
Can
I
4.5.
with
YES
–factor
there
are
from
the
3.
Form
conversion
factors.
23
to
“cancel”
out
moles
and
you atoms.
significant
digits.
convert
directly
from
moles
to
original problem.
6.02 x 10 atoms
=give
1 mole
atoms?
6.02 x 1023 atoms
1 m0le
1 mole
6.02 x 1023 atoms
23 Fe atoms
6.02
x
10
10.0 moles Fe x
= 6.02 x 1024 Fe atoms
1 mole Fe
1
Factor Label – It’s back…..
How many molecules are in 12.1 g of
H2SO4?
Molar mass = 2(1.00)g + 32.00 g + 4(16.00) g = 98.09 g.
1. NO
Ask– yourself
the
question
– Can I
You
will
need
two
conversion
5. 6.
Use
conversion
factors
that
will
allow
you
to
4.
Start
with
your
“given”
from
the
Cancel
out
units
and
calculate
using
2.
Calculate
Molar
Mass
of
H
SO
.
3. convert
Form
conversion
factors.
2
4moles
directly
from
grams
to
factors.
Grams
to
moles
and
“cancel”
out
grams
and give you moles and moles
original
problem.
significant
digits.
molecules?
to molecules.
to give
you molecules.
1
16
8
Molar mass =
6.02+ 4(16.00
x 1023 molecules
2(1.01) +.32.07
g) = 98.09 g
1 mole
1 mole 98.09 g
98.09 g 1 moleS 6.02 x 1023 molecules
H
1.00794
O
32.066
1 mole
15.9994
23 molecules
6.02
x
10
1
mole
12.1 g H2SO4 x
=
x
98.09 g H2SO4
1 mole
1
7.42 x 1022 molecules H2SO4
Factor Label – It’s back…..
How many atoms are in 210.0 g of
Molar
mass
= 2(1.00)g + 32.00 g + 4(16.00) g = 98.09 g.
H
SO
?
2
4
1.
Ask
yourself
the
question
–allow
Can
I to
How
do
we
go
from
molecules
to
atoms?
Count
the
number
of
atoms
in
one
4.
Start
with
your
“given”
from
the
NO
–
You
will
need
three
conversion
factors.
5. Use
conversion
factors
that
will
you
2.3.Calculate
Molar Mass
of H2SO4.
Form
conversion
factors.
molecule
of
sulfuric
acid.
convert
directly
from
grams
toand
6. original
Cancel
units
and
calculate
using
Grams
to
moles,
moles
to
molecules
andmoles
“cancel”
outout
grams
and
give
you
moles
problem.
2H
+
1
S
+
4
O
=
7
atoms
in
1
molecule
of
H
SO
so…..
2
4
molecule
to
atoms.
atoms
for
a
molecule?
significant
digits.
to give
you molecules.
7 Molar
atomsmass = .
1 molecule H2SO4
1
16
8
1 molecule
7
atoms
1 mole
6.02
x 1023 molecules
2(1.01) +H.32.07
g) = 98.09 g
2SO
4+ 4(16.00
1 mole 98.09 g
1 mole
98.09 g 1 mole 6.02 x 1023 molecules
H
S
O
1.00794
32.066
15.9994
23 molecules
210.0 g H2SO4 x 1 mole
6.02
x
10
x 7 atoms H2SO4 =
x
1
1 mole
1 molecule H2SO4
98.09 g H2SO4
9.022 x 1024 atoms H2SO4
What conditions need to exist to
use the conversion 1 mole – 22.4 L?
Standard Temperature and Pressure - STP
Standard Temperature
Standard Pressure
0 oC
1 atm or 760 torr
or 101.3 KPa
At these conditions 1 mole of any gas has
a volume of 22.4 L.
*We will learn how to convert gases at other conditions in the
Gas Law Unit.
Factor Label – It’s back…..
How many molecules are in 15.7 L of Iron(II) Oxide?
NOyourself
– you will
need
two
conversion
4.
Use
conversion
factor
that
allow
you
1.
Ask
the
question
– will
Can
I
5.3. Cancel
Start
2. Form
with
outconversion
units
your and
“given”
calculate
factors.
from
using
the
factors.
Liters
toand
mole
and
mole
to
to
“cancel
out
moles
give
you
atoms.
convert
directly
from
liters
to
original
significant
problem.
digits.
molecules
molecules?
6.02 x 1023 molecules
1 m0le
1 mole
6.02 x 1023 molecules
1 mole
22.4 L
23
15.7 L FeO x 1 mole FeO x 6.02 x 10 molecules FeO
1
1 mole FeO
22.4 L FeO
22.4 L
1 mole
=
4.22 x 1023 FeO molecules