1 - Gas Laws (terms)

Pressure

\- force acting upon a specific area

Volume

\- dimensional space occupied by gas

Temperature

\- measure of warmth or coldness of a body

\- measure of the average kinetic energy of the particles in an obbject

K=C+273

\- formula for converting Celsius to Kelvin

C=K-273

\- formula to convert Kelvin to Celsius

Kelvin

\- all gas calculations must use ___

\- standard unit for temperature in gas

Quantity

\- increased in mole

Kinetic Theory of Matter

\- gasses consist of large number of molecules (atoms) that are moving in continuous, random motion

atm

\- unit of atmosphere

torr

\- unit of torr

mm Hg

\- unit for millimeters of mercury

psi

\- unit for pounds per square inch

kPa

\- unit for kilopascals

1\.00 atm

\- standard pressure of atmosphere

760 torr

\- standard pressure of torr

760 mm Hg

\- standard pressure of millimeters of mercury

14\.7 psi

\- standard pressure of pounds per square inch

101\.3 kPa

\- standard pressure of kilopascals

L

\- unit for liters

mL

\- unit for milliliters

m^3

\- unit for cubic meter

cm^3

\- unit for cubic centimeter

1L

\- standard volume of liter

1000mL

\- standard volume for milliliter

0\.001m^3

\- standard volume for cubic meter

1000cm^3

\- standard volume for cubic centimeter

Boyle’s Law

\- at constant temperature for a mixed mass, the absolute pressure and volume of a gas are inversely proportional

Charles’s Law

\- when the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be directly related

GayLussac’s Law

\- the pressure of a fixed amount of gas at constant volume is directly proportional to its temperature

Combined Gas Law

\- combines Boyle’s, Charles’s, and GayLussac’s Laws into one

\- when the amount of gas is kept constant, this law describes the relationship between pressure, volume, and temperature

Ideal Gas Law

\- combines the separate gas laws into one equation that allows to solve for all variables