Home
Class 11
CHEMISTRY
A pure gas that is 14.3% hydrogen and 85...

A pure gas that is `14.3%` hydrogen and `85.7%` carbon by mass has a density of `2.5g L^(-1)` at `0^(@)C` and 1 atm pressure. What is the molecular formula of the gas :

A

`CH_(2)`

B

`C_(2)H_(4)`

C

`C_(4)H_(8)`

D

`C_(6)H_(12)`

Text Solution

Verified by Experts

The correct Answer is:
C
`% "mol Simples ratio"`
`C" " 85.7 " "85.7//12 = 7.14" "7.14// 7.14 = 1 " "1`
`H " "14.3" " 14.3//1 = 14.3" " 14.3//7.14 = 2 " "2`
`:.` Emperical formal `=CH_(2)`
`:. PMw = DRT`
`Mw = (DRT)/(P) = (2.5 xx 0821 xx 273)/(1) =56`
`n = ("molecular wt")/("Ewt") = (56)/(14) = 4`
Molecular formula `= n xx E.F`
`= 4 xx CH_(2)`
`= C_(4) H_(8)` .
Promotional Banner

Similar Questions

Explore conceptually related problems

An organic compound was found to have contained carbon = 40.65%, hydrogen = 8.55% and Nitrogen = 23.7%. Its vapour - density was found to be 29.5. What is the molecular formula of the compound?

An alloy of gold and silver contains 38.5% silver by mass and has a density of 14.6 g.mL^(-1) . What is the molar concentration of silver in this alloy :

A 5% solution of anhydrous CaCI_(2) at 0^(@)C developed 15 atm osmotic pressure. What is the degree of dissociation of CaCI_(2) .

An acid of molecular mass 104 contains 34.6% carbon, 3.85% hydrogen and the rest is oxygen. Calcualte the molecualr formula of the acid.

A solution containing 12.0% sodium hydroxide by mass has a density of 1.131 g//mL . What volume of this solution contains 5.00 mol of NaOH :