Answer:
1. Sulfur (S) and Oxygen (O)
2. empirical formula (mole ratio)
3. or Sulfur Dioxide
Solution:
G: 50.05% S ; 49.95%O
R: empirical formula
A: find the mole ratio
S:
assume 100g:
50.05% S = 50.05g S
49.95% O = 49.95g O
convert from mass to moles:
[tex]50.05g S(\frac{1 mol S}{32.07g S}) = 1.5605 mol S[/tex]
[tex]49.95g O(\frac{1 mol O}{16.00g O}) = 3.1219 mol O[/tex]
solve for mole ratio:
*1.5605mol is the lowest amongst the moles so use it as the divisor
[tex]\frac{1.5605 molS}{1.5605} = 1[/tex]
[tex]\frac{3.1219 molO}{1.5605} = 2[/tex]
use the mole ratio to write the formula:
[tex]SO_{2}[/tex]
A: The empirical formula is [tex]SO_{2}[/tex] more commonly known as sulfur dioxide
