# Problem: 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.

###### FREE Expert Solution

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.

97% (136 ratings) ###### Problem Details

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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Based on our data, we think this problem is relevant for Professor Morkowchuk's class at UVA.