Ideal Gas Law Crash Course Chemistry #12

as Volume decreases, Pressure increase (as particles hit the container wall more frequently) inversely proportional

• P x V = constant (k)-Volume Relationship
• P / V = constant (k)
• P x T = constant (k)
• P / T = constant (k)

PV = k. A principle that describes the relationship between the pressure and volume of a gas at constant temperature.

• Boyle's Law
• Charles' Law
• Avogadro's Law
• Newton's Law
• Ideal Gas Law

Volume/temperature = constant. (as long as pressure stays the same). V/T = b

• Charles' law
• Boyle's Law
• Avogadro's Law
• Newton's Law
• Ideal Gas Law

Volume/Amount of moles = constant. V/n = a

• Avogadros Law
• Charles' Law
• Boyle's Law
• Newton's Law
• Ideal Gas Law

PV = nRT Most gases ideally behave in the same predictable way. If we know don't know one of these variables, we can calculate it if we know all the others (Pressure, Volume, moles, or Temp). We need to choose the correct constant R depending on the type of measurements being used.

• Ideal Gas Law
• Boyle's Law
• Charles' Law
• Avogadro's Law
• Newton's Law

pressure equation

• pressure = force/area
• force = pressure/area
• area = pressure X force
• (force x pressure)/area

The total space a group of particles take-up. For gas laws we use unit measurements in Liters.

• Volume
• Mass
• Area
• Temperature

R = 8.3145 L kPa/ K mol.

• R = Universal Gas Constant
• R = pressure x area
• R = force/area
• R = force/pressure

Measure of the average kinetic energy of all the particles in an object. Must use units of Kelvin or the calculations will not work.

• Temperature
• Volume
• Mass
• Force

Tags

NGSS.HS-PS3-4

conditions of 0.00°C and 1 atm pressure (or 101.325 kPa, 14.7 psi, or 760 Torr/mmHg)

• STP (standard temperature and pressure)
• Ideal Gas Law
• Universal Gas Constant
• Boyle's Law
• Charles' Law