What is the empirical formula of the sulfur-oxygen compound?

Question

A chemist heats 50g of sulfur under controlled conditions to produce a sulfur-oxygen compound. The mass of the sulfur-oxygen compound is 100g. What is the empirical formula of the sulfur-oxygen compound?

Answer 1

Empirical formula = weight/g-atomic wt of each element. and then expressed as a ratio.


For sulfur, 50/32= 1.56
For oxygen, 50/16 = 3.12

So O:S=2:1, and the empirical formulas is SO2

Answer 2

Formula Sulfur

Answer 3

The Sulfur compound is SO2 - 1 atom of Sulfur with 2 atoms of Oxygen.

Sulfur atomic mass = 32 = 1 mole = 32 gram/mole
Oxygen atomic mass = 16 (x 2 = molecular mass)
= 32 = 1 mole = 32 gram/mole

SO2 mol.mass = 32 + 32 = 64

50g 'S' = 50/32 = 1.5625 mol.
100g 'SO2' = 100/64 = 1.5625 mol

If 50g = Sulfur (S atom), then 50g = Oxygen (O2 molecule)

Sulfur - Oxygen compound = SO2

Answer 4

i anticipate that the possibilities given confer with mass. enable's anticipate that we've precisely one hundred. g of this compound. Then, the shape of grams of each ingredient (sulfur and oxygen) is 50. grams each. next, enable's locate the shape of moles of "atoms" (no longer molecules) of each ingredient in this compound with assistance from dividing the mass of each ingredient with assistance from its gram-atomic mass: S = (50. g) / (32.064 g/mol) = a million.5593812 mol O = (50. g) / (15.9994 g/mol) = 3.1251171 mol because the numbers of moles of each ingredient at the instantaneous are not entire numbers, enable's divide one and all with assistance from the smaller of both: S = (a million.5593812 mol) / (a million.5593812 mol) = a million O = (3.1251171 mol) / (a million.5593812 mol) = 2.0040751 ? 2 Now, the ratio of sulfur to oxygen atoms in this compound is a million : 2, so the empirical formulation for this compound is SO2.