Step 1. Calculate mass % C
= 1.18 g C
% C = 46.83
Step 2. Calculate mass % H
= 0.11 g H
% H = 4.49 %
Step 3. Calculate mass % S
= 0.845 g S
% S = 20.41 %
Step 4. Calculate mass % N
= 0.505 g N
% N = 8.92 %
Step 5. Calculate mass % O
This will just be what is left of 100 %.
Step 6. Calculate the moles of each
Assume 100 g → the mass percent will be equal to the mass.
Then calculate moles based on molar mass.
A 2.52-g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur was burned in excess oxygen to yield 4.23 g of CO2 and 1.01 g of H2O. Another sample of the same compound, of mass 4.14 g, yielded 2.11 g of SO3. A third sample, of mass 5.66 g, was burned under different conditions to yield 2.27 g of HNO3 as the only nitrogen-containing product.
Calculate the empirical formula of the compound.
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