contestada

An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combustion of 5.50 g of this compound produced 8.07 g of carbon dioxide and 3.30 g of water.

Required:
a. How many moles of carbon, C, were in the original sample?
b. How many moles of hydrogen, H, were in the original sample?

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Respuesta :

maacastrobr

Answer:

a. 0.183 mol C

b. 0.366 mol H

Explanation:

Assuming total combustion, all of the carbon in the unknown compound turned into carbon dioxide, COâ‚‚.

So first we calculate the COâ‚‚ moles produced, using its molecular weight:

  • 8.07 g COâ‚‚ ÷ 44 g/mol = 0.183 mol COâ‚‚

This means in the unknown compound there were 0.183 moles of carbon, C.

Conversely, all of the hydrogen in the unknown compound turned into water, Hâ‚‚O.

Calculating the Hâ‚‚O moles:

  • 3.30 g ÷ 18 g/mol = 0.183 mol Hâ‚‚O

We multiply the water moles by two, as there are 2 H moles per Hâ‚‚O mol:

  • 0.183 * 2 = 0.366 mol H.

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