Question

O. 200 mole of a hydrocarbon undergo complete combustion to give 35.2g of carbon dioxide and 14.4g of water as the only products. What is the molecular formula of the hydrocarbon?

Answer 1

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C(a)H(b)O(c) ------> x CO2 + y H2O  

0.2 moles of the hc gives 0.8 moles of co2 and h2o  

So 1 mole gives 4 moles of water and co2  

CaHbOc --------> 4CO2 + 4H2O  

So molecular formula is C4H8O12

Answer 2

Answer:

the molecular formula of the hydrocarbon is

Explanation:

Here options are not give so i have added options

A) C₂H₄

B) C₂H₆

C) C₄H₄

D) C₄H₈

Given

O. 200 mole of a hydrocarbon undergo complete combustion

to give 35.2g of carbon dioxide

14.4g of water as the only products

To find

the molecular system of the hydrocarbon?

Solution

CxHy + O₂ --> CO₂ + H₂O

number of moles of CO₂: 35.2g / (12+16+16)gmol-1

=0.8 mol.

Same number for H₂O.

CxHy has 0.2 mol, meaning 4 less (ratio) than CO₂ ad H₂O, so:

CxHy + O₂ --> 4CO₂ + 4H₂O

Balancing the Cs, and following the molar ratio, x is 4, and y is 8. The O₂ reactant can be balanced to make it have 6, therefore:

C₄H₈ + 6O₂ --> 4CO₂ + 4H₂0

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