Atoms
The number of atoms in 12.0 g of Carbon-12.
6.02 x 1023 atoms of Carbon
The number of moles in 6.94 g of Li.
1 mol Li
The mass in grams from 0.0474 mol of Fe.
2.65 g Fe
The number of molecules from 18.0 g of H2O.
6.02 x 1023 molecules H2O
This is the molar mass of Xenon.
131.3 g/mol
The number of atoms in 0.5000 mol of Mg.
3.011 x 1023 atoms Mg.
The number of moles in 4.068 x 1024 atoms of Pb.
6.755 mol Pb
The number of grams in 6.50 moles of Cu.
413 g Cu
The number of formula units in 0.688 mol of AgNO3.
4.14 x 1023 fu AgNO3
This is the two-step process to convert the mass of a substance to its number of particles (list the process).
Divided by molar mass then multiply by Avogadro's Number
The number of atoms in 6.05 g of Mg.
1.05 x 1024 atoms Mg
The number of moles in 0.00750 g Ag
6.95 x 10-5 mol Ag
The mass of Zn from 0.00818 mol of Zn.
0.535 g Zn
The number of formula units in 5.1 g of TiO2.
3.8 x 1022 fu TiO2
This is the molar mass of C6H11OH.
100 g/mol C6H11OH
The number of atoms from 0.250 mol of Sulfur.
1.51 x 1023 atoms S
The number of moles in 2.25 x 1025 atoms of Zn.
37.4 mol Zn
Mass in grams in 4.50 x 1012 atoms of Cl.
2.65 x 10-10 g Cl
The number of molecules in 693 g of C10H22.
2.94 x 1024 molecules C10H22
12 g of Carbon-12 is equivalent to just one of these.
1 mole
The number of atoms in 0.02550 g of Pt.
7.872 x 1019 atoms Pt
The number of moles in 150 g of Sulfur.
4.7 mol S
The mass of 8.42 x 101 atoms of Br.
0.00112 g Br
The number of molecules in 1.25 mol of O2.
1.51 x 1024 molecules O2
Formula Units are the units used for this kind of chemical compound.
Ionic Compounds