Home
Class 12
CHEMISTRY
When 1.2 g of Sulphur is melted with 15 ...

When 1.2 g of Sulphur is melted with 15 g of naphthalene, the solution freezes at`77.2^(@)C`. What is the molar mass of this form of Sulphur?
Deta for napthalene:
Melting point (f.pt.) ` 80.0^(@)C`
Freezing point depression constant `K_(f) 6.80Km^(-1)`

A

`180g "mol"^(-1)`

B

`190g "mol"^(-1)`

C

`260g "mol"^(-1)`

D

`450g "mol"^(-1)`

Text Solution

AI Generated Solution

To solve the problem, we need to determine the molar mass of sulfur when it is mixed with naphthalene, which causes a depression in the freezing point. Here’s a step-by-step solution: ### Step 1: Understand the Given Data - Mass of sulfur (solute) = 1.2 g - Mass of naphthalene (solvent) = 15 g - Freezing point of pure naphthalene = 80.0 °C - Freezing point of the solution = 77.2 °C - Freezing point depression constant (Kf) for naphthalene = 6.80 K·kg⁻¹ ...
Promotional Banner

Similar Questions

Explore conceptually related problems

When 1.20g of sulphur is melted with 15.00g of naphthalene, the solution freezes at 77.2^(@)C . What is the moalr mass of this from of sulphur. Data for Napthalene Melting point, m.p 80^(@)C Freezing point depression constant, k_(f) = 6.80^(@)Cm^(-1)

15 g of a solute in 100 g of water makes a solution of freeze at -1^(@)C.30g of a solute in 100 g of water will give a depression in f.pt. equal to:

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 freezing point of a solution containing 4.8 g of a compound in 60 g of benezene is 4.48 ^(@) C what is the molar mass of the compound ? (k_(f)=5.1 Km^(-1) , freezing point of benezene =5.5^(@)C )

In 100 g naphthalene 2.56 g sulphur is added boiling point of solution (solid) decreases by 0.68^(@)C , atomicity of sulphur is ( K_(f) of naphthalene=6.8 Km^(-1) )

A solution containing 8.0 g of nicotine in 92 g of water-frezes 0.925 degrees below the normal freezing point of water. If the freezing point depression constant K_(f) = -1.85^(@)C mol^(-1) then the molar mass of nicotine is -

C_6H_6 freezes at 5.5^(@)C . The temperature at which a solution 10 g of C_4H_(10) in 200g of C_6H_6 freeze is __________ ""^(@)C . (The molal freezing point depression constant of C_6H_6 is 5.12^(@)C//m .)