Question

5.6 g of an organic compound on burning with excess

of oxygen gave 17.6 g of CO2, and 7.2 g of H,O. The
organic compound is :​

Answer 1

Answer:organic compound is :​ C₄H₈

Explanation: The equation of the reaction of the organic compound burning with excess oxygen gives us the general equation as

C xHy + 1/2(x+ y/2 )O₂ → xCO₂ + y/2H₂O

We first find the number of moles of CO₂ and H₂O

Number of moles of CO₂= Mass/ molar mass

= 17.6g/ 44g/mol ( 12+ 16 x2)

=0.4 moles

Number of moles of H₂O= Mass/ molar mass

= 7.2g/ 18g/mol ( 1 X 2+ 16)

=0.4 moles

From the reaction , we can see that

x = 0.4

and
`(y)/(2)`= 0.4 such that y= 0.4 x 2= 0.8

Their ratios become

`(x)/(y)` =
`(0.4)/(0.8)`=
`(4)/(8)`

Therefor the organic compound CxHy = C₄H₈

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