Gas Laws and Kinetic Theories Quiz

Kinetic Theories of Matter

• Matter is composed of tiny particles (atoms or molecules) in constant, random motion.
• Kinetic energy of these particles increases with temperature, leading to increased particle motion.
• Particles collide with each other and the container walls, transferring energy.

Graham's Law of Effusion/Diffusion

• Effusion is the escape of a gas through a tiny opening.
• Diffusion is the spontaneous mixing of gases.
• The rate of effusion and diffusion of a gas is inversely proportional to the square root of its molar mass.

Boyle's Law

• At constant temperature, the pressure of a fixed amount of gas is inversely proportional to its volume.
• P1V1 = P2V2

Charles's Law

• At constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute temperature.
• V1/T1 = V2/T2

Avogadro's Law

• Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.

General Gas Law

• Combines Boyle's, Charles's, and Avogadro's laws to relate pressure, volume, temperature, and amount of gas.

Ideal Gas Law

• PV = nRT
• P = pressure
• V = volume
• n = number of moles
• R = ideal gas constant
• T = absolute temperature(Kelvin)

Deviation from the Ideal Gas Law

• Ideal gas law assumes gas particles have negligible volume and no attraction between them.
• Real gases deviate from ideal behavior at high pressure and low temperature due to particle volume and intermolecular forces.

Dalton's Law of Partial Pressures

• Total pressure of a mixture of gases is the sum of the partial pressures of the individual gases.
• P_total = P₁ + P₂ + P₃...