What is the elevation in boiling point for a one molal solution of a solute in a solvent called?

$A$ 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. $(K_b = 2.5 \ K \ kg \ mol^{-1})$

Which of the following formulas correctly gives the value of the ebullioscopic constant $(K_{b})$?

For water,$K_b = 0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $200 \ mL$ of water,at what temperature will the resulting solution boil at $1 \ atm$ pressure (in $^oC$)?

If $K_b$ denotes the molal elevation constant of water,then the boiling point of an aqueous solution containing $36 \ g$ of glucose (molar mass $= 180 \ g \ mol^{-1}$) per $dm^3$ is:

Give the unit for the molal elevation constant in boiling point.