Moles/Empirical Formula
how to find # of particles (quantity)
# of given moles x 6.02x10^23 particles/mol
how to find mass
# of moles x molar mass g/mol
volume
1 mole=22.4 liters
mass
6.02x10^23 particles of given substance
25 grams of HF = how many moles
1.25
67.2 L = how many moles
3
A compound with an empirical formula of C2OH4 and molar mass of 132 grams per mole. Determine the molecular formula
C6O3H12
Empirical Formula of hydrocarbon is C3H4. the molecular weight was calculated to be 121 amu. What is its molecular formula?
C: 3(12.011)=36.00 amu H: 4(1.008)=4 amu C3H4 empirical formula weight: 40 amu 121 amu/40 amu = 3 C: 3*3=9 H: 4*3=12 Molecular Formula: C9H12
Empirical Formula of C5H10O5
CH2O
Whole Number Multiple (helps you figure out the molecular formula)
Molecular Weight/Empirical Formula Weight Then you multiply the answer to each of the parts of the empirical formula
molecule
compound with covalent bonds nonmetal/metal 2+ capital letters
formula units
compounds with ionic bonds metal bonded with nonmetal
how to find volume
given # of moles x 22.4 l/mol
how to find moles (quantity)
given # of particles/6.02x10^23 particles/mol
how to find moles
given mass/molar mass g/mol
how to find moles (volume)
given volume/22.4 l/mol
Avogadro's #
one mole of anything= 6.02x10^23
atoms
pure elements only 1 capital letter
molar mass
atomic mass found on periodic table
particles
atoms, molecules, formula units
How many atoms are there in 3.2 moles of iron
1.9 x 10^24
How many molecules are there in 3.2 moles of sulfur dioxide, SO2?
1.9 x 10^24
5 moles = how many liters
112
88.4 moles of NI3 = how many grams
34,891.48
6.6 moles of ZnO = how many grams
534.6
Percent of Carbon in C2H6
80%
65.5% C, 5.5% H, and 29%O - determine the empirical formula
C3H3O
A compound has a molecular formula of C8H8O2, what is it's empirical formula
C4H4O
mole
unit used with very small particles 6.02x10^23 mass, volume, quantity can be determined
formula mass
when finding mass of compound
