Home
Class 12
CHEMISTRY
Y g of a non-volative Oranic substance o...

Y g of a non-volative Oranic substance of molecular mass M is dissolved in 250g benzene Molal elevation contant of bezene is `K_(b)` . Elevation in its B.P is given by

A

`(M)/(K_(b)Y)`

B

`(4K_(b)Y)/(M)`

C

`(K_(b)Y)/(4M)`

D

`(K_(b)Y)/(M)`

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Similar Questions

Explore conceptually related problems

1.0 g of a non-electrolyte solute (molar mass 250 g "mol"^(-1) ) was dissolved in 51.2 g of benzene. If the freezing point depression constant of benzene is 5.12 K kg "mol"^(-1) , the lowering in freezing point will be

When 0.9 g of a non-volatile solute was dissovled in 45 g of benezene, the elevation of boiling point is 0.88^@C . If K_b for benezene is 2.53 K kg "mol"^(-1) , Calculate the molar mass of solute.

1.00 g of a non-electrolyte solute dissolved in 50g of benzene lowered the freezing point of benzene by 0.40 K. The freezing point depression constant of benzene is 5.12 K kg mol^(-1) . Find the molar mass of the solute.

What is K_b , if 0.5 g of solute ( molar mass 100g/mol) in 25g of solvent showed an elevation of 1^@ C in B.P.

The boiling point of benzene is 353.23 K. When 1.80 g of a non-volatile solute was dissolved in 90 g of benzene, the boiling point is raised to 354.11 K. Calculate the molar mass of the solute. K_(b) for benzene is 2.53" K kg mol"^(-1) .

2.0g of a non-electrolyte dissolved in 100g of benzene lowers the freezing point of benzene by 1.2K. The freezing pont depression constant of benzene is 5.12 K kg mol^(-1) . The molar mass of the solute is

2g of a non-electrolyte solute dissolved in 200 g of water shows an elevation of boiling point of 0.026^(@)C. K_(b) of water is 0.52 K . "mole"^(1) kg then the molecular weight of solute is x xx100 . What is the value of 'x'?

When some amount of non-volatile solute is dissolved in a solvent to prepare a dilute solution, the vapour pressure of the solvent is lowered and it is directly proportional to the mole fraction of solvent in the solution . Relative lowering in vapour pressure is equal to mole fraction of solute . Elevation in boiling point of solvent is a collgative property like lowering in vaour pressure of solvent in solution , K_(b) i.e., molal elevation constant is calculated by the formula, K_(b)=DeltaT_(b)// molality and also by the expression, K_(b)=RT_(b)^(2)//1000l_(v) where T_(b) is boiling point of solvent and I_(v) is latent heat of vapourisation for 1 gm solvent . Abnormal elevation is boiling point =iX elevation in boiling point in ideal solution where i=van't Hoff factor Molal elevation (K_(b))

When some amount of non-volatile solute is dissolved in a solvent to prepare a dilute solution, the vapour pressure of the solvent is lowered and it is directly proportional to the mole fraction of solvent in the solution . Relative lowering in vapour pressure is equal to mole fraction of solute . Elevation in boiling point of solvent is a collgative property like lowering in vaour pressure of solvent in solution , K_(b) i.e., molal elevation constant is calculated by the formula, K_(b)=DeltaT_(b)// molality and also by the expression, K_(b)=RT_(b)^(2)//1000l_(v) where T_(b) is boiling point of solvent and I_(v) is latent heat of vapourisation for 1 gm solvent . Abnormal elevation is boiling point =iX elevation in boiling point in ideal solution where i=van't Hoff factor Lowering in vapour pressure in an experiment was found to be x mm of Hg. It is : Lowering in vapour pressure in an experiment was found to be x mm of Hg. It is

When some amount of non-volatile solute is dissolved in a solvent to prepare a dilute solution, the vapour pressure of the solvent is lowered and it is directly proportional to the mole fraction of solvent in the solution . Relative lowering in vapour pressure is equal to mole fraction of solute . Elevation in boiling point of solvent is a collgative property like lowering in vaour pressure of solvent in solution , K_(b) i.e., molal elevation constant is calculated by the formula, K_(b)=DeltaT_(b)// molality and also by the expression, K_(b)=RT_(b)^(2)//1000l_(v) where T_(b) is boiling point of solvent and I_(v) is latent heat of vapourisation for 1 gm solvent . Abnormal elevation is boiling point =iX elevation in boiling point in ideal solution where i=van't Hoff factor Relative lowering in vapour pressure :