Home
Class 10
CHEMISTRY
0.8 g sample of gaseous hydrocarbon occu...

0.8 g sample of gaseous hydrocarbon occupying 1.12 L at STP, when completely burnt in air produced 2.2 g of carbon dioxide and 1.8 g of water. Calculate.
(a) the mass of the compound
(b) the molecular formula of the compound, and
(c) the volume of oxygen at STP required for combustion.

Text Solution

Verified by Experts

Hint :
Calculate the molar mass of the compound at STP using mass - volume relationship .
(b) Calculate precentage composition and molecular formula of the compound.
(c ) Write the balanced chemical equation and calculate the volume of oxygen required for the combustion .
Ans : (i) 16 (ii) `CH_(4)` (iii) 2.24 L
Promotional Banner

Topper's Solved these Questions

  • EMPIRICAL AND MOLECULAR FORMULA

    CENGAGE CHEMISTRY|Exercise OLYMPIAD AND NTSE LEVEL EXERCISES|10 Videos

  • EMPIRICAL AND MOLECULAR FORMULA

    CENGAGE CHEMISTRY|Exercise CONSOLIDATED EXERCISE |1 Videos

  • HYDROCARBONS

    CENGAGE CHEMISTRY|Exercise OLYMPIAD AND NTSE LEVEL EXERCISES|10 Videos

Similar Questions

Explore conceptually related problems

A sample of gaseous hydrocarbon occupying 1.12 "litre" at NTP , when completely burnt in air produced 2.2 g CO_(2) and 1.8 g H_(2)O . Calculate the weight of hydrocarbon taken and the volume of O_(2) at NTP required for its combustion.

The volume of oxygen at STP required to burn 2.4 g of carbon completely is :

The volume of O_(2) at STP required for the complete combustion of 4g CH_(4) is

44g of a sample on complete combustion given 88g CO_2 and 36g of H_2 O. The molecular formula of the compound may be :