Gas Laws Foldable
First, fold your paper
in half like this.
Not this.
You need six “flaps.”
Cut only the top half of the
folded paper.
There are six flaps of information.
Label the top of your flaps like
below:
Under flap 1 – Boyle’s Law
P↑
P↓
V↓
V↑
Pressure and volume
vary inversely when
temperature remains
constant
1
2
3
4
Under flap 1 – Boyle’s Law
P1V1 = P2V2
•Pressures need to
have the same units
•Volumes need to
have the same units
1
2
3
4
Under flap 2 – Charles’ Law
T↑
V↑
T↓
V↓
Temperature and
volume vary
directly when
pressure remains
constant
1
2
3
4
Under flap 2 – Charles’s Law
V1
=
T1
V2
T2
V1T2 = V2T1
•Volumes need to have the same units
•Temperatures both need to be in K
(not °C or °F)
1
2
3
4
Under flap 3 – Gay-Lussac’s Law
T↑
T↓
P↑
P↓
Pressure and
temperature vary
directly when volume
remains constant
1
2
3
4
Under flap 3 – Gay-Lussac’s Law
P1
=
T1
P2
T2
P1T2 = P2T1
•Pressures need to have the same
units
•Temperatures both need to be in K
(not °C or °F)
1
2
3
4
Under flap 4 – Combined Gas
Law
1
Pressure, temperature,
and volume can all
change with the
following equation.
2
3
4
Under flap 4 – Combined Gas Law
P1V1
P2V2
=
T1
T2
P1V1T2 = P2V2T1
•Pressures need to have the same units
•Volumes need to have the same units
•Temperatures both need to be in K
(not °C or °F)
1
2
3
4
Under flap 5 –
Dalton’s Law of Partial Pressures
The total pressure of a gas is
equal to the sum of the
partial pressures of the
individual gases
3
4
5
6
Under flap 5 –
Dalton’s Law of Partial Pressures
PT = P1 + P2 + P3 + …
•All pressures must have the
same units
© Carey Munoz
3
4
5
6
Under flap 6 – Ideal Gas Law
A law relating pressure,
temperature and
volume of an ideal gas
3
4
5
6
Under flap 6 – Ideal Gas Law
PV = nRT
•P is pressure
(atm, kPa, mmHg, torr)
•V is volume (mL, L)
•n is number of moles
•R is Ideal Gas Law Constant
•T is temperature (K)
Choose the R value based on the
units for pressure.
3
4
5
6
Back side of
foldable –
Some helpful
conversion factors
& constants
Standard Pressures
1 atm
760 mm Hg
101.325 kPa
101,325 Pa
14.7 psi
760 torr
Common Volume
Conversions
1 L = 1000 mL
1 cc = 1 mL = 1 cm3
Ideal Gas Constants (R)
R= 0.0821 L*atm/mol*K
R = 8.31 L*kPa/mol*K
R = 62.364 L*mmHg/mol*K
R = 62.364 L*torr/mol*K
Temperature Conversions
K = °C + 273
°C = (°F – 32)
1.8