Unit
1:
Gas
Laws
Day
3
Name:
____________________________
Date:
______________________________
2.5
Ideal
Gas
Law
As
discussed
in
class,
all
of
the
simple
gas
laws
can
be
combined
to
form
one
ideal
gas
law.
Ideal
Gas
Law
P
is
pressure
in
kPa
V
is
volume
in
L
n
is
the
#
of
moles
of
gas
mol
R
is
the
gas
constant
8.31
(kPa
L)/(mol
K)
T
is
the
temperature
in
Kelvin
The
ideal
gas
law
can
be
used
to
find
an
unknown
variable
given
________
of
the
others
conditions
are
known.
The
ideal
gas
law
follows
the
________________
theory
of
_______________
and
makes
some
ideal
assumptions
that
are
not
always
true.
Refer
to
pg
100
for
the
exceptions.
eg.
1
How
many
moles
of
N2
and
O2
are
there
in
this
tire?
2.5.1
Molar
Mass
of
a
Gas
It
is
possible
to
determine
the
molar
mass
of
a
gas
using
the
ideal
gas
law.
Simply
replace
the
number
of
moles
____
by
the
variables
_____________.
eg.
2
A
gas
at
STP
has
a
volume
of
68.5
L
and
10
g.
Identify
this
gas.
Unit
1:
Gas
Laws
Day
3
2.6
General
Gas
Law
The
general
gas
law
is
used
to
calculate
the
new
conditions
of
a
gas
when
at
least
two
variables
change.
It
is
a
combination
of
the
all
the
simple
gas
laws.
eg.
3
At
SATP,
0.150
mol
of
water
vapour
occupies
a
volume
of
55.0
mL.
What
is
the
new
temperature
in
degrees
Cesius
(0C)
if
0.030
mol
of
water
vapour
is
removed
while
increase
the
pressure
to
115.0
kPa
and
decreasing
the
volume
to
40.0
mL.
Homework
Problems
1.
If
3.7
moles
of
propane
are
at
a
temperature
of
28oC
and
are
under
154.2
kPa
of
pressure,
what
volume
does
the
sample
occupy?
(60
L)
2.
A
sample
of
carbon
monoxide
at
57oC
and
under
0.67
atm
of
pressure
takes
up
85.3
L
of
space.
What
mass
of
carbon
monoxide
is
present
in
the
sample?
(59
g
CO)
3.
At
–45oC,
71
g
of
fluorine
gas
take
up
6843
mL
of
space.
What
is
the
pressure
of
the
gas,
in
kPa?
(517.6
kPa)
4.
At
971
mm
Hg,
145
g
of
carbon
dioxide
have
a
volume
of
34.13
dm3.
What
is
the
temperature
of
the
sample,
in
oC?
(‐112oC)
5.
At
137oC
and
under
a
pressure
of
3.11
atm,
a
276
g
sample
of
an
unknown
noble
gas
occupies
13.46
L
of
space.
What
is
the
gas?
(Radon)
6.
During
a
laboratory
experiment,
you
put
an
unknown
compound
into
some
water.
You
observe
a
bubbling
reaction.
With
the
help
of
a
syringe,
you
remove
the
gas
produced.
Consider
the
following
data:
Mass
of
the
140
mL
syringe:
23.47
g
Mass
of
the
syringe
with
140
mL
of
the
gas:
23.72
g
Temperature
in
the
lab:
298.0
K
Pressure
in
the
room:
101.0
kPa
Which
of
the
following
is
most
likely
the
identity
of
the
gas
produced
and
collected?
(CO2)