chemistry unit 3

mole

the amount of a substance in 12g of C-12

avogadro’s number

the number of units in a mole 6.02 × 10²³

molas mass

the mass in grams of 1 mole of a substance

AMU

atomic mass unit

stoichiometry

the study of relative amounts of substances in chemical reactions

reactant : reactant ratio

calculate the amount of reactants required to react completely

product : product

predict the amount of byproduct and storage requirement

limiting reactant

the reactant that is used up first

excess reactant

the reactant that is leftover

theoretical yield

the maxmim theoretically amount of a product that can be made

actual yield

the actual amount of product produced

percent yield

actual yield divided by the theoretical yield as a percent

equation for percent yield

%yield = actual yield / theoretical yield × 100

boyle’s law

pressure and volume are inversely proportional

boyle’s law equation

P1V1 = P2V2

lussac gay’s law

pressure and temperature are directly proportional

lussac gay’s law equation

P1/T1 = P2/T2

charles’ law

volume and temperature are directly proportional

charles’ law equation

V1/T1 = V2/T2

combined gas law

describes the relationship between pressure, volume, and temperture

combined gas law equation

P1V1/T1 = P2V2/T2

partial pressure

the pressure a gas would exert if it were the only gas in the container

dalton’s law

the total pressure is equal to the sum of all partial pressures

dalton's law equation

Ptotal = P1 + P2 + P3 + … Pn

avogadro’s law

more gas molecules will take up more space

stp

0°c, 1 atm

molar volume

22.4 l

ideal gas law equation

V1/n2 = V2/n2

r (atm)

0.0821

r (torr)

62.396

r (kpa)

8.317

k conversion

°c + 273

ideal gas

no volume, no attraction

pressure is inversely related to

volume

temperture is inversely related to

moles

volume is inversely related to

pressure

moles is inversely related to

temperature

stp volume

22.4 l

units for P

atm, torr, kpa

unit for V

liters

units for T

kelvin

units for N

mole

how to derive ideal gas law

volume is directly proportional to moles

the mole concept will most likely be used in

determining how many ozone molecules are lost in the atmosphere

how does a mole of Mg compare with a mole of Fe?

they have the same number of atoms.

which laws combine to form the ideal gas laws?

charles, avogadro, and boyle’s laws

which statement can best be concluded from the ideal gas law?

the product of pressure and volume of an ideal gas is proportional to the absolute temperature.

which describes the volume of 1 mol of gas at standard temperature and pressure?

the volume is the same for any gas.

pressure is increased from 2 atm to 3 atm. what law is this?

boyle’s law

if a gas is moved from a large container to a small container but its temperature and number of moles remain the same, what would happen to the pressure of the gas?

it would increase

if the pressure, volume, and temperature of a gas are known, which can most likely be found by using the ideal gas law?

the molar amount of the gas