0.15 molal solution of a substance boils at 373.23 K. Calculate molal elevation constant of water, (Given boiling point of water=373.15K)

Molal elevation constant is elevation in boiling poind produced by

The boiling point of 0.15 molal aqueous solution of an unknown solute is 373.23 K at 1 atm. The molal elevation constant of water is ______ K kg mol ^(-1)

The depression of freezing point of a solvent (b.p:303 K) for a particular solution is 0.153 K. Calculate the molal elevation constant if the boiling point of the solution is 304.52 K .(K_(f) =1.68 K kg mol ^(-1))

The molal elevation constant is the ratio of the elevation of boiling point to _____.

Define ebullioscopic constant or molal elevation constanct or boiling point elevation constant. State the units of Kb.

A 5% aqueous solution (by mass) of cane sugar (molar mass 342 g/mol) has freezing point of 271K. Calculate the freezing point of 5% aqueous glucdse solution if freezing point of water is 273.15K.

If molality of the dilute solution is doubled the value of molal depression constant (K_(f)) will be ______.

3.795 g of sulphur is dissolved in 100 g of carbon disulfide. This solution boils at 319.81K. What is the molecular formula of sulphure in solution? The boiling point of the solvent is 319.45K. (Given that Kb for CS2 = 2.42 K kg mol(-1) and atomic mass of S = 32)