Overview
This lecture introduces three fundamental gas laws—Boyle's Law, Charles's Law, and Gay-Lussac's Law—comparing their relationships among pressure, volume, and temperature.
Boyle's Law
- The mass of gas is constant in Boyle's Law.
- Pressure and volume are inversely proportional: as pressure increases, volume decreases, and vice versa.
- Density and pressure are directly proportional: as pressure rises, density increases.
- Key formula: ( P_1V_1 = P_2V_2 ) or ( \frac{P_1}{V_1} = \frac{P_2}{V_2} ).
- Pressure (P) times volume (V) equals a constant (K).
Charles's Law
- Pressure is constant in Charles's Law.
- Temperature and volume are directly proportional: as temperature increases, volume increases.
- Density is inversely proportional to temperature: as temperature increases, density decreases.
- Key formula: ( \frac{V_1}{T_1} = \frac{V_2}{T_2} ).
- Volume (V) divided by temperature (T) equals a constant (K).
Gay-Lussac's Law
- Mass is fixed and volume is constant in Gay-Lussac's Law.
- Pressure and temperature are directly proportional: as temperature increases, pressure increases.
- Key formula: ( \frac{P_1}{T_1} = \frac{P_2}{T_2} ).
Key Terms & Definitions
- Pressure (P) — The force exerted by gas particles per unit area.
- Volume (V) — The amount of space the gas occupies.
- Temperature (T) — A measure of the average kinetic energy of gas particles.
- Density — Mass per unit volume of a substance.
- Proportionality Constant (K) — A constant value representing the relationship between variables in each gas law.
Action Items / Next Steps
- Review the formulas for all three gas laws.
- Practice applying each law to sample problems involving gas pressure, volume, and temperature.