{ [ 8.0(g) / 63.55(g/molCu) ] / 2(2Cu per S) } * 32(g/molS) = 2.0 g Sulfur.
All dimensions are in 'brackets ( ) directly following the number.
The maximal mass is 30 moles sulfur dioxide.
The mass of a formula unit of cuprous sulfide (Cu2S) is 159.152 g/mol.
Cu(I) sulfide has the formula Cu2S. Thus the mass in grams of a single formula unit is 63.5 x 2 = 127 for two coppers32.1 x 1 = 32.1 for one STotal = 159.1
A chunk of sulfur has a volume of 5.95 cm3. What is the mass of this sulfur? (Density of sulfur = 2.07 g/cm3.)
50
The maximal mass is 30 moles sulfur dioxide.
One definition of a mole is the sum of the average atomic weights (mass) of a compound. In this case 2 Copper + 1 Sulfur = (2 * 63.55) + (1 * 32.07) = 159.17 grams per mole. So 22 g / 159.17 g/mole = 0.14 mole of Cu2S
The mass of a formula unit of cuprous sulfide (Cu2S) is 159.152 g/mol.
Cu(I) sulfide has the formula Cu2S. Thus the mass in grams of a single formula unit is 63.5 x 2 = 127 for two coppers32.1 x 1 = 32.1 for one STotal = 159.1
A chunk of sulfur has a volume of 5.95 cm3. What is the mass of this sulfur? (Density of sulfur = 2.07 g/cm3.)
Sulfur is a non metallic element. Mass number of it is 32.
Heating sulfur (yellow form, S8) gives initially a red liquid which solidifies as a rubbery mass. This is termed plasic sulfur. This slowly reverts back to the yellow form. These changes are considered to be physical changes although the molecular form changes (it is still sulfur) from S8 to a metastable polymeric plastic sulfur. There is often ignition of the sulfur - to form sulfur dioxide this is most definitely a chemical change.
the percent sulfur by mass in so3 is 40.050%
Atomic number for sulfur: 16
69
50
69