CH 11 Gas Laws

It is a theory that explains the behaivor of gases by examining individual molecules. Below is the theory.

• 1. Gases consist of individual molecules or atoms in constant random motion
• 2. Particles are widely spaced
• 3. Particles do not attract or repel each other
• 4. Particles collide with each other and with the sides of it's container.
• 5. Temperature is expressed in Kelvin (degrees celcius + 273) which indicates kinetic energy in particles.

REVIEW THIS DIAGRAM

• Pressure = atm
• Volume = L
• Mass = mol
• temperature = Kelvin (degrees celcius + 273)

P₁V₁=P₂V₂

• V₁ / T₁ = V₂ / T₂

P₁ / T₁ = P₂ / T₂

P₁V₁ / T1 = P₂V₂ / T₂

V₁ / n₁ = V₂ / n2

• Avagadro's Law also states that 1 mole of any gas has a volume of 22.4L This is called the molar gas volume.

Standard Temperature (273 K) and Pressure (1 atm).

PV= nRT

P_total = P₁ + P₂ + P₃ +...

In essence the total pressure is the sum of all the pressures of all gases in a container.

• 1. Convert given mass to moles.
• 2. Use mole to mole ratio to convert unknown to moles.
• 3. Use the other givens and the unknown in mole and plug them into the Ideal Gas Law (PV=nRT) to solve for unknown.