Gas Law Chemistry Test

Gas Laws

100

Graham's Law

Smaller molar masses effuse faster

(Rate 1/Rate 2) = (Square root of Molar Mass 2/Square root Molar Mass 1)

200

Boyle's Law Formula

P1 x V1 = P2 x V2

300

Combined Gas Law Formula

(P1 x V1)/(T1) = (P2 x V2)/(T2)

400

Charles' Law Formula

V1/T1 = V2/T2

500

Gay Lussac's Law

P1/T1 = P2/T2

Converting

100

22^o = _ K

295K

200

-60.0^o = _ K

213K

300

390.0K = _^oC

117^oC

400

1 atm = _ kPa

101.3kPa

500

760 mmHg = _ psi

14.7 psi

Converting + Vocab

100

760 mmHg = _ Torr

760 Torr

200

Ideal Gas Law

PV = nRT

300

Properties of Gases

- The volume occupied by a gas is mostly empty space

- Gases are very compressible

- Gases are subject to conditions of T, P, V, and Moles

400

Kinetic Molecular Theory (KMT)

A theory that explains the behavior of matter based on the idea that all particles are in constant motion

- Solids: Particles are tightly packed and vibrate in place

- Liquids: Close but move fluidly around

- Gases: Far apart and have little volume

500

Conversion Units for Pressure

- atm

- Torr

- mmHg

- kPa

Vocab

100

What two values of R are most often used for solving Ideal Gas Law equations?

R = 0.0821 L (used when pressure is in ATMOSPHERES and volume in LITERS)

R = 8.314 J (used when pressure is in PASCALS (Pa) and volume in CUBIC METERS (m³) ) 

200

Ideal Gases VS Real Gases

- Ideal gases are HYPOTHETICAL and real gases exist in NATURE

- Real gases have volume while ideal gases don't

- Real gases have intermolecular forces while ideal gases don't