The molal elevation constant is the ratio of the elevation in $B.P.$ to

$A$ solution of a nonvolatile solute is obtained by dissolving $3.5 \ g$ of solute in $100 \ g$ of solvent. The boiling point elevation is $0.35 \ K$. Calculate the molar mass of the solute. $(K_b = 2.5 \ K \ kg \ mol^{-1})$

$A$ solution containing $0.1050 \ g$ of a substance in $15.84 \ g$ of ether has a boiling point $1 \ ^\circ C$ higher than that of pure ether. What is the molar mass of the substance? [Given: Molar elevation constant for ether per $100 \ g = 21.6$]

If $10 \ g$ of a solute (molar mass $= 100 \ g/mol$) is dissolved in $100 \ g$ of water,then the molal elevation constant $K_b$ of the solvent will be equal to:

$A$ solution containing $2 \ g$ of a non-volatile solute in $20 \ g$ of water boils at $373.52 \ K$. The molecular mass of the solute is $....... \ g \ mol^{-1}$. (Nearest integer) Given,water boils at $373 \ K$,$K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$.

The solution containing $3 \ g$ urea (molar mass $60 \ g \ mol^{-1}$) per $dm^3$ of water and another solution containing $4.5 \ g$ of solute $A$ per $dm^3$ of water boil at the same temperature. What is the molar mass of $A$?