The combustion of a hydrocarbon A gives 0.66 g of carbon dixode and 0.36 g of water. The empirical formula of the hydrocarbon is:

C_{3} H_{10}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C_{3} H_{4}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C_{3} H_{8}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

C_{6} H_{8}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B $C_{3} H_{8}$
$44 g o f {C O}_{2} \to 1 m o l o f c a r b o n$

$∴ 0.66 g o f C O_{2} \to 0.66 / 44 = 0.015 m o l C$

$18 g o f H_{2} O \to 2 m o l o f H y d r o g e n$

$∴ 0.36 g o f H_{2} O \to \frac{2}{18} \times 0.36 = 0.04 m o l H$

$m o l a r r a t i o o f C : H i s 0.015 : 0.04$
$C : H = 1 : 8 / 3 = 3 : 8 E m p i r i c a l f o r m u l a = C_{3} H_{8}$

Suggest Corrections

Similar questions

0.72 g

3.08 g

C O_{2}

0.72

3.08

C O_{2}

A gaseous hydrocarbon gives upon combustion 0.72 g. of water and 3.08 g. of CO₂. The empirical formula of the hydrocarbon is:

0.20

0.66

C O_{2}

Join BYJU'S Learning Program