An unknown compound contains only carbon, hydrogen, and oxygen (cxhyoz). combustion of 5.00 g of this compound produced 7.33 g of carbon dioxide and 3.00 g of water. how many moles of carbon, c, were in the original sample?

Answer : The number of moles of carbon in the original sample were 0.166 moles.

Explanation :

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of

Mass of

We know that:

Molar mass of carbon dioxide = 44 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 7.33 g of carbon dioxide, of carbon will be contained.

Now we have to calculate the moles of carbon.

Moles of Carbon =

Therefore, the number of moles of carbon in the original sample were 0.166 moles.

the dependant variable is spilled water

the independent is the heat