An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combust

Question

An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combustion of 7.00 g of this compound produced 10.3 g of carbon dioxide and 4.20 g of water.
How many moles of Carbon were in the original sample? How many moles of Hydrogen were in the original sample? An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combustion of 7.00 g of this compound produced 10.3 g of carbon dioxide and 4.20 g of water.
How many moles of Carbon were in the original sample? How many moles of Hydrogen were in the original sample?
How many moles of Carbon were in the original sample? How many moles of Hydrogen were in the original sample?

Explanation / Answer

PART A

The reaction would then be CxHyOz + ?O2 -----> ?CO2 + ? H2O

You know the mass of the compound = 7.00g

You know the mass of the CO2 = 10.3 g

You know the mass of the H2O = 4.20 g

moles=mass/molar mass.

mass of CO2 = 10.3 g and molar mass of CO2 = 44.009 g/mol, there is 1 mol C in CO2

moles C in the original sample = 10.3 / 44.009 g/mol = 0.234

moles C in the original sample = 0.234 mol

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PART B

The reaction would then be CxHyOz + ?O2 -----> ?CO2 + ? H2O

You know the mass of the compound = 7.00g

You know the mass of the CO2 = 10.3 g

You know the mass of the H2O = 4.20 g

mass of H2O = 4.20 g and molar mass of CO2 = 18.02 g/mol, there is 2 mol H in H2O, hence

moles H = 2 x 4.20/18.02 g/mol= 0.466

moles H in the original sample = 0.466 mol

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