Elevation in Boiling Point of the Solvent

Define elevation in boiling point. How can you calculate the molecular mass of a non-volatile solute with it ?

The molal boiling point elevation constant depends upon

State if molal boiling point elevation constant depends upon the type of solvent.

The boiling point of benzene is $353.23\mathrm{K}$. When $1.80 \mathrm{g}$ of a non-volatile, non-ionisable solute was dissolved in $90\mathrm{g}$ of benzene, the boiling point raised to $354.11 \mathrm{K}$. Calculate molar mass of the solute in ${\mathrm{gmol}}^{-1}$( ${\mathrm{K}}_{\mathrm{b}}$ for benzene= $2.53 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$)

(Report your answer upto 1 decimal value)

Latent heat of vaporization for a liquid solvent is $500 \mathrm{cal} {\mathrm{g}}^{-1}.$ Let the boiling point be ${\mathrm{T}}_{\mathrm{b}} \mathrm{K}.$ Find the value of ${\mathrm{K}}_{\mathrm{b}}$ of the solvent in $\mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. 

The molal elevation constant is the ratio of the elevation in boiling point to:

Which of the following aqueous solutions should have the highest boiling point?

The unit of an ebullioscopic constant is ______.

Boiling point of a solvent is $80.2°\mathrm{C}$. When $0.419 \mathrm{g}$ of the solute of molar mass $252.4 \mathrm{g} {\mathrm{mol}}^{-1}$ was dissolved in $75 \mathrm{g}$ of the solvent, the boiling point of the solution was found to be $80.256°\mathrm{C}$. Find the molal elevation constant.

Calculate the mass in grams of an impurity of molar mass $100 \mathrm{g} {\mathrm{mol}}^{-1}$ which would be required to raise the boiling point of $50 \mathrm{g}$ of chloroform by $0.30 \mathrm{K}$. $({\mathrm{K}}_{\mathrm{b}}$ for chloroform = $3.63 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1})$

If mass is expressed in gram then ${\mathrm{K}}_{\mathrm{b}}$ is given by.

Which of the following aqueous solution will have the boiling point ${102.2}^{o}C?$ The molal elevation constant for water is $2.2 K kg mo{l}^{-1}.$

If the elevation in boiling point of a solution of 10 g of solute (mol. wt. = 100) in 100 g of water is $\mathrm{\Delta }{\mathrm{T}}_{\mathrm{b}}$ , the ebullioscopic constant of water is

The boiling point elevation constant for toluene is $3.32\mathrm{ }\mathrm{K}\mathrm{ }\mathrm{k}\mathrm{g}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$, the normal boiling point of toluene is ${\mathrm{110.7 }}^{\mathrm{o}}\mathrm{C}$. The enthalpy of vaporization of toluene would be nearly:

0.15 g of a substance dissolved in 15 g of a solvent is boiled at a temperature higher by ${0.216}^0\mathrm{C}$ than that of the pure solvent. Find out the molecular weight of the substance. $\left({\mathrm{K}}_{\mathrm{b}} \mathrm{f}\mathrm{o}\mathrm{r}\mathrm{ }\mathrm{s}\mathrm{o}\mathrm{l}\mathrm{v}\mathrm{e}\mathrm{n}\mathrm{t}\mathrm{ }\mathrm{i}\mathrm{s}\mathrm{ }2.16\mathrm{ }\mathrm{K}.\mathrm{k}\mathrm{g}.{\mathrm{mol}}^{-1}\right)$

Which of the following solution has the highest elevation in boiling point ?

A solution containing 12.5 g of non-electrolyte substance in 175 g of water gave boiling point elevation of 0.70 K. Calculate the molar mass of the substance. Molal elevation constant $\left({\mathrm{K}}_{\mathrm{b}}\right)$ for water $0.52\mathrm{ }\mathrm{K}\mathrm{ }\mathrm{k}\mathrm{g}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ ?

The molal elevation constant of water is $0.52℃$. The boiling point of 1.0 modal aqueous KCl solution (assuming complete dissociation of KCl), therefore, should be

Pressure cooker reduces cooking time for food because

If 0.15 g of a solute, dissolved in 15 g of solvent, is boiled at a temperature higher by $0.216\text{℃}$ than that of the pure solvent. The molecular weight of the substance (molal elevation constant for the solvent is $2.16\text{℃})$ is