Chemistry Chapter 13

Boyle’s Law

Boyle’s Law

P1V1 = P2V2

Charles’s Law

V1/T1 = V2/T2

Gay-Lussac’s Law

P1/T1 = P2/T2

Combined Gas Law

P1V1/T1 = P2V2/T2

Dalton’s Law of Partial Pressures

Ptotal = P1 + P2 + P3 + P4 + …

STP atm

1.00

STP kPa

101.325

STP mmHg/torr

760

STP temp (K)

273

Ideal Gas Law

PV = nRT

Ideal Gas Law + mass and molar mass

PVM = mRT

density of a gas

m/V

Avogadro’s Principle

22.4 L/ mol

expands

____________ to assume the shape and volume of its container

flows

readily ____________

straight lines

particles only move in ____________

compressible

molecules far apart but ____________

few

____________ attractive forces between particles

volume

space occupied by a gas sample

mL, L, cm^3, dm^3

volume units

1 cm^3

1 mL = ____________

1dm^3

1 L = ____________

temperature

a measure of the average kinetic energy of a group of particles

thermometer

measurement tool for temperature

kelvin (K)

temperature unit

amount

number of moles of the substance

mol

amount unit

pressure

force per unit area caused by the collision of the gas molecules with the walls of the container

manometer

measurement tool for pressure

pascal (Pa), atmosphere (atm), torr, millimeter of mercury (mmHg)

pressure units

kinetic molecular theory

a model that uses particle motion and interparticle forces to properties of different states of matter

no volume

individual gas particles have almost ____________

inter particle

gas particles have no ____________ forces

constant random

gas particles are in ____________ motion

elastic

collisions are ____________, no energy lost

average kinetic energy

all gases have the same ____________ at a given temperature

high temp and low pressure

real gases behave like ideal gases at:

avogadro’s principle

equal volume of all gases measured at the same temperature and pressure contain the same number of particles