Elevation in Boiling Point of the Solvent

$18 \mathrm{g}$ of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ dissolved in $1 \mathrm{kg}$ of water is heated to boiling. The boiling point (in $\mathrm{K}$) measured at $1 \mathrm{atm}$ pressure is closest to [Ebullioscopic constant, ${\mathrm{K}}_{\mathrm{b}}$ for water is $0.52 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. Consider absolute zero to be $-273.15°\mathrm{C}$]

The molal boiling point elevation constant depends upon

A solution of $122 \mathrm{g}$ of benzoic-acid in $1000 \mathrm{g}$ of benzene shows a boiling point elevation of $1.4°$$.$ If the solute is dimerized to an extent of $80\%$$,$ the boiling point of pure benzene will be_________  (Molar enthalpy of vaporization of benzene $=7.8\mathrm{kcal}.{\mathrm{mol}}^{-1}$ )

The elevation in boiling point of a solution of $10 g$ of a binary electrolyte (of molecular mass $100$) in $100 \mathrm{g}$ of water is ${\mathrm{\Delta T}}_{\mathrm{b}}$. Then the value of ${\mathrm{K}}_{\mathrm{b}}$ for water is

$1$ molal aqueous solution of an electrolyte ${\mathrm{A}}_2{\mathrm{B}}_3$ is $60\%$ ionised. The boiling point of the solution at $1 \mathrm{atm}$ is _____ K. (Rounded-off to the nearest integer)  [Given ${\mathrm{K}}_{\mathrm{b}}$ for $\left({\mathrm{H}}_2\mathrm{O}\right)=0.52 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$]

The elevation of boiling point of $0.10 \mathrm{m}$ aqueous ${\mathrm{CrCl}}_3{\mathrm{xNH}}_3$ solution is two times that of $0.05 \mathrm{m}$ aqueous ${\mathrm{CaCl}}_2$, solution. The value of $\mathrm{x}$ is..........

[Assume $100\%$ ionisation of the complex and ${\mathrm{CaCl}}_2$, coordination number of $\mathrm{Cr}$ as $6$, and that all ${\mathrm{NH}}_3$ molecules are present inside the coordination sphere]

Molal elevation constant is the elevation in boiling point produced by

The boiling point (in ${}^{\circ }\mathrm{C}$) of $0.1$ molal aqueous solution of ${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O}$ at $1$ bar is closest to: [Given: Ebullioscopic (molal boiling point elevation) constant of water, $\left.{\mathrm{K}}_{\mathrm{b}}=0.512 \mathrm{K} {\mathrm{kgmol}}^{-1}\right]$

A solution is formed by addition of some amount of sucrose (Molecular weight $=342$ ) in $100 \mathrm{g}$ water such that difference between boiling point and freezing point of solution is found to be $101.19°\mathrm{C}.$ Mass of sucrose in solution is $\mathrm{Y}\times {10}^{-1} \mathrm{g}$. Calculate the value of $\mathrm{Y}$?

$\left[{\mathrm{K}}_{\mathrm{f}}=1.86 \mathrm{K}-\mathrm{kg}/\mathrm{mol}\right.$and $\left.{\mathrm{K}}_{\mathrm{b}}=0.52 \mathrm{K}-\mathrm{kg}/\mathrm{mol}\right]$

The molal elevation constant for water is $0.52$. What will be the boiling point of $2$ molar sucrose solution at $1 \mathrm{atm}$ pressure? (Assume that the boiling point of pure water is $100 \mathrm{℃}$)

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)

The boiling point of $0.001 \mathrm{M}$ aqueous solutions of $\mathrm{NaCl}, {\mathrm{Na}}_2{\mathrm{SO}}_4, {\mathrm{K}}_3{\mathrm{PO}}_4$ and ${\mathrm{CH}}_3\mathrm{COOH}$ should follows the order.

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 $\mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. 

Which of the following is incorrect: 

If Van't Hoff factor for $\mathrm{KCl}$ is $1.8.$ What is the boiling point of $0.75 \mathrm{m}$ solution of $\mathrm{KCl}$ in water ${\mathrm{K}}_{\mathrm{b}}=0.5°\mathrm{Ckg}/\mathrm{mol}$?

Which compound has the highest value of ${\mathrm{K}}_{\mathrm{b}}$ ?

The molal elevation constant of water $=0.52 \mathrm{K} {\mathrm{m}}^{-1}$. The boiling point of $1.0 \mathrm{molal}$ aqueous $\mathrm{KCl}$ solution (assuming complete dissociation of $\mathrm{KCl}$ ) should be:

Elevation of boiling point was found to be $0.52°\mathrm{C}$, when $8\mathrm{g}$ of a compound $\text{'}\mathrm{X}\text{'}$ was dissolved in $200\mathrm{g}$ of water. The molecular mass of $\text{'}\mathrm{X}\text{'}$ will be $\left[{\mathrm{K}}_{\mathrm{b}\left({\mathrm{H}}_2\mathrm{O}\right)}=0.52 {\mathrm{Km}}^{-1}\right]:$

The boiling point of $0.2 \mathrm{mol} {\mathrm{kg}}^{-1}$ solution of $\mathrm{X}$ in water is greater than equimolal solution of $\mathrm{Y}$ in water. Which one of the following statements is true in the case?