Home
Class 12
CHEMISTRY
It has been found that 0.290 g of an org...

It has been found that 0.290 g of an organic compound containing C, H and O on complete combustion yielded 0.66 g of `CO_2` and 0.27 g of `H_2O`. The vapour density of the compound is found to be 29.0. Determine the molecular formula of the compound.

Text Solution

Verified by Experts

The correct Answer is:
60
0.6 g of the organic compound can give `112/22400` moles of `N_2` gas. Thus, `10^(-2)` moles of N-atom are present in 0.6 gm. of the compound. So minimum molar mass of the compound is 60 gram/mole.
Promotional Banner

Topper's Solved these Questions

  • JEE MAIN REVISION TEST - 18

    VMC MODULES ENGLISH|Exercise CHEMISTRY - SECTION 2|5 Videos

  • JEE MAIN REVISION TEST - 13

    VMC MODULES ENGLISH|Exercise CHEMISTRY (SECTION 2)|5 Videos

  • JEE MAIN REVISION TEST - 19

    VMC MODULES ENGLISH|Exercise CHEMISTRY|26 Videos

Similar Questions

Explore conceptually related problems

0.290 g of an organic compound containing C, H and O gave on combustion 0.270 g of water and 0.66 g of CO_(2) . What is empirical formula of the compound.

0.2 g off an organic compound contains C, H and O. On combustion, it yields 0.15 g CO_(2) and 0.12" g "H_(2)O . The percentage of C, H and O respectively is

0.45 g of an orgainc compound containing only C, H and N on combustion gave 1.1 g of CO_(2) and 0.3 g of H_(2) O . What is the percentage of C, H and N in the orgainc compound.

0.29 g of an organic compound on combustion gave 0.66 g of CO_2 and 0.27 g of H_2 O . The percentage of carbon and hydrogen in the given compound respectively are

12.8 gm of an organic compound containing C, H and O and undergoes combustion to produce 25.56 gm CO_(2) and 10.46 gm of H_(2)O . What is the empirical formula of compound.

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 :

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 :

The empirical formula of a compound is CH_2O and its vapour density is 30. The molecular formula of the compound is:

The molecular mass of a compound having empirical formula C_2H_5O is 90. The molecualr formula of the compound is:

0.2 g of a monobasic acid gave 0.5 g of CO_2 and 0.089 g of H_2 O . 0.122 g of the same acid requires 10 mL of 0.1 N NaOH for complete neutralisation. Determine the molecular formula of the compound.

Knowledge Check

  • 0.2 g off an organic compound contains C, H and O. On combustion, it yields 0.15 g CO_(2) and 0.12" g "H_(2)O . The percentage of C, H and O respectively is

    A
    `C=15%,H=20%,O=65%`
    B
    `C=10%,H=8.2%,O=81.8%`
    C
    `C=12.2%,H=8.8%,O=79%`
    D
    `C=20%,H=6.66%,O=73.34%`

  • 0.29 g of an organic compound on combustion gave 0.66 g of CO_2 and 0.27 g of H_2 O . The percentage of carbon and hydrogen in the given compound respectively are

    A
    `10.3, 62.1`
    B
    `44.6, 10.7`
    C
    `62.1, 10.3`
    D
    `10.7, 44.6`