Gas law calculations show up constantly in GCSE, A-Level and AP Chemistry exams, and this deck of 20 flashcards covers every formula you'll need. Starting with Boyle's, Charles's and Gay-Lussac's laws individually, the deck builds up to the combined gas law an...
Gas law calculations show up constantly in GCSE, A-Level and AP Chemistry exams, and this deck of 20 flashcards covers every formula you'll need. Starting with Boyle's, Charles's and Gay-Lussac's laws individually, the deck builds up to the combined gas law and the full ideal gas equation (PV = nRT), including how to work with STP and molar volume. You'll also cover Avogadro's law, Dalton's law of partial pressures, and Graham's law of effusion, alongside the underlying assumptions of kinetic molecular theory that explain why these laws work. A few cards address common student misconceptions, like why temperature must always be converted to kelvin, and how real gases deviate from ideal behaviour at high pressure or low temperature. Each flashcard pairs the formula with a plain-English explanation, so you understand not just what to calculate but why the relationship holds.
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Flip through all 20 cards in interactive study mode.
At constant temperature, the pressure and volume of a gas are inversely proportional:
π
1
π
1
=
π
2
π
2
P
1
β
V
1
β
=P
2
β
V
2
β
.
At constant pressure, the volume of a gas is directly proportional to its absolute temperature:
π
1
/
π
1
=
π
2
/
π
2
V
1
β
/T
1
β
=V
2
β
/T
2
β
.
At constant volume, the pressure of a gas is directly proportional to its absolute temperature:
π
1
/
π
1
=
π
2
/
π
2
P
1
β
/T
1
β
=P
2
β
/T
2
β
.
π
1
π
1
π
1
=
π
2
π
2
π
2
T
1
β
P
1
β
V
1
β
β
=
T
2
β
P
2
β
V
2
β
β
β combines Boyle's, Charles's and Gay-Lussac's laws into one relationship.
Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
π
π
=
π
π
π
PV=nRT, where
π
=
0.0821
R=0.0821 LΒ·atm/(molΒ·K), relating pressure, volume, moles and temperature.
0Β°C (273.15 K) and 1 atm (or per IUPAC's newer definition, 0Β°C and 100 kPa).
22.4 litres per mole.
Gas particles are in constant random motion, have negligible volume, experience no intermolecular forces, and undergo perfectly elastic collisions.
The total pressure of a gas mixture equals the sum of the partial pressures of each individual gas:
π
π‘
π
π‘
π
π
=
π
1
+
π
2
+
β¦
P
total
β
=P
1
β
+P
2
β
+β¦.
The pressure a single gas in a mixture would exert if it alone occupied the entire container volume.
A hypothetical gas that perfectly obeys the gas laws. Real gases deviate at high pressure and low temperature, where intermolecular forces and molecular volume become significant.
Density = molar mass Γ· 22.4 L/mol at STP; heavier gases are denser under the same conditions.
The rate of effusion of a gas is inversely proportional to the square root of its molar mass: lighter gases effuse faster.
Average kinetic energy is directly proportional to absolute temperature (in kelvin), regardless of the gas identity.
Pressure doubles, per Boyle's law, since
π
β
1
/
π
Pβ1/V.
Gas laws rely on direct proportionality to absolute temperature; Celsius includes negative values that would break the proportional relationship.
The pressure exerted by a vapour in equilibrium with its liquid (or solid) phase at a given temperature.
Rearrange
π
π
=
π
π
π
PV=nRT to
π
=
π
π
π
π
n=
RT
PV
β
, using consistent units (atm, L, K).
Molecules are further apart (reducing intermolecular forces) and moving faster (making their own volume relatively negligible), approximating ideal behaviour.
