Combined Gas Laws and Properties of Gases

A set of 41 flashcards covering key concepts and formulas related to gas laws, properties of gases, and colligative properties.

Combined Gas Law

P1V1/T1 = P2V2/T2, relates pressure, volume, and temperature for a fixed amount of gas.

Molar Volume at STP

22.4 L/mol for an ideal gas.

STP Definition

Standard Temperature and Pressure: 1 atm and 273 K.

Ideal Gas Law

PV = nRT; R = 0.0821 L·atm·mol^-1·K^-1.

Effect of doubled P and T

Volume (V) remains unchanged.

Variable 'n' in PV = nRT

Number of moles of gas.

Effect of halving V on P

Pressure (P) doubles if temperature (T) and moles (n) are constant (Boyle's Law).

Effect of doubled T on V

Volume (V) doubles if pressure (P) and moles (n) are constant (Charles' Law).

Average Kinetic Energy and Temperature

Directly proportional to absolute temperature (Kelvin).

Elastic Collision Definition

A collision with no net loss of kinetic energy.

Heat Equation

q = m·c·ΔT; where m is mass (g), c is specific heat (J/g·°C), and ΔT is temperature change.

Heat of Fusion Formula

q = m·Hf; calculates heat required to melt or freeze a substance.

Heat of Vaporization Formula

q = m·Hv; calculates heat required to boil or condense a substance.

Gas Density Formula

D = PM/RT; relates density to pressure, molar mass, gas constant, and temperature.

Effect of Increasing T on P at Constant Volume

Increases pressure (P); directly proportional.

Definition of % (w/v)

grams of solute per 100 mL of solution × 100%.

Definition of % (w/w)

grams of solute per 100 g of solution × 100%.

Definition of % (v/v)

mL of solute per 100 mL of solution × 100%.

Molarity Definition

M = moles of solute / liters of solution.

Dilution Equation

M1V1 = M2V2; relates concentrations and volumes before and after dilution.

Temperature Effect on Solubility of Solids

Solubility increases with temperature.

Temperature Effect on Solubility of Gases

Solubility decreases with temperature.

Henry's Law

Higher pressure increases gas solubility in liquids.

Electrolyte Definition

A substance that forms ions in water; e.g., NaCl.

Strong vs Weak Electrolyte

Strong electrolytes dissociate nearly completely; weak electrolytes only partially dissociate.

Direction of Osmosis

Solvent moves from lower solute concentration to higher solute concentration.

Osmolarity (Osm) Definition

Osm = (number of ions, n) × molarity M.

Osmotic Pressure Formula

π = n·M·R·T; relates osmotic pressure to number of moles, molarity, gas constant, and temperature.

Hypertonic vs Hypotonic vs Isotonic

Hypertonic: higher solute concentration; Hypotonic: lower solute concentration; Isotonic: equal solute concentrations.

Boiling Point Elevation Formula (Water)

ΔTb = n·Kb·M; Kb = 0.52 °C·kg·mol^-1.

Freezing Point Depression Formula (Water)

ΔTf = n·Kf·M; Kf = 1.86 °C·kg·mol^-1.

Liters Occupied by 2.00 mol of Ideal Gas at STP

44.8 L.

Liters of H2O Formed from 10.0 L H2

10.0 L H2O produced from reaction with O2.

Using PV = nRT to Solve for n (Moles)

n = PV / RT.

Moles from Molarity and Volume

n = M·V; where M is molarity and V is volume in liters.

Van't Hoff Factor for NaCl in Colligative Properties

n = 2; NaCl dissociates into two ions.

Heat (q) for 50.0 g Water

q = m·c·ΔT; results in 5230 J.

Grams of CO2 in 11.2 L at STP

22.0 g of CO2.

Heat (q) for 50.0 g Water with Temperature Change

q = 523 J; results in 5230 J.

Boiling Point Elevation for 0.50 M NaCl (n=2)

ΔTb = 0.52 °C.

Freezing Point Depression for 0.50 M NaCl (n=2)

ΔTf = 1.86 °C.