Home
Class 12
CHEMISTRY
If a solution containing 0.072 g atom of...

If a solution containing 0.072 g atom of sulphur in 100 g of a solvent `(k_f=7.0)` gave a freezing point depression of `0.84 @_C`, the molecular formula of sulphur in the solutions is :

A

`S_6`

B

`S_7`

C

`S_8`

D

`S_9`

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Similar Questions

Explore conceptually related problems

A solution containing 25.6 g of sulphur, dissolved in 1000 g of naphthalene whose melting point is 80.1^(@)C gave a freezing point lowering of 0.680^(@)C . Calculate the formula of sulphur ( K_(f) for napthalene = 6.8 K m^(-1) )

The boiling point of a solution of 5g of sulphur in 100g of carbon disulphide is 0.474^(@)C above that of pure solvent. Determine the molecular formula of sulphur in this solvent. The boiling point of pure carbon disulphide is 47^(@)C and its heat of vaporisation is 84 calories per gram.

2.56 f of suphur in 100 g of CS_(2) has depression in freezing point of 0.010^(@) K_(f)=0.1^(@) (molal)^(-1) . Hence atomicity of sulphurin the solution is

A solution containing 6.8 g of a non-ionic solute in 100 g water was found to freeze at 272.07 K . The freezing point depression constant mass of the solute is ______.

5g sulphur is present in 100 g of CS_(2). DeltaT_(b) of solution 0.954 and K_(b) is 4.88. The molecular formula of sulphur is

If solution containing 0.15 g of solute dissolved in 15 g of solvent boils at a temperature higher by 0.216^(@)C than that of pure solvent, the molecular mass of the substance is (K_(b)=2.16^(@)C)

(a) A solution containing 0.5g of naphithalene in 50g C Cl_(4) yield a boiling point elevation of 0.4K , while a solution of 0.6g of an unknown solute in the same mass of the solvent gives a boiling point elevation of 0.65K . Find the molar mass of the unknown solute. (b) The boiling point of a solution of 0.1g of a substance in 16g of ether was found to be 0.100^(@)C higher that of pure ether. What is the molecular mass of the substance. K_(b) (ether) =2.16K kg "mol"^(-1)

Normal freezing point of a solvent is 150^@C . A 0.5 molal solution of urea in the above solvent causes a freezing point depression of two degrees. Calculate the molal depression constant