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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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Combustion Analysis concept. You can view video lessons to learn Combustion Analysis. Or if you need more Combustion Analysis practice, you can also practice Combustion Analysis practice problems.
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Based on our data, we think this problem is relevant for Professor Morkowchuk's class at UVA.