Calculate the molal elevation constant of water if molar enthalpy of vaporisation of water at 373 K is 40.585 kJ/mol.

Open in App

Solution

Suggest Corrections

Similar questions

Q. Calculate the molal elevation constant,

K_{b}

for water and the boiling of 0.1 molal urea solution. Latent heat of vaporisation of water 9.72 kcal

m o l^{1}

at 373.15K.

Q. Calculate the molal elevation constant,

k_{b}

for water and the boiling point of 0.1 molal urea solution. Latent heat of vaporisation of water is 9.72 kcal mol

^{- 1}

at 373.15 K.

Assuming that, water vapour is an ideal gas the internal energy change (ΔU)(ΔU) when 11 mol of water is vaporized at 11 bar pressure and 100o100o C will be:

[given: molar enthalpy of vaporisation of water at

1

bar and

373

= 41

m o l^{- 1}

and

R = 8.3

K^{- 1}

m o l^{- 1}

]

Standard enthalpy of combustion of $C H_{4}$ is $- 890 k J m o l^{- 1}$ and standard enthalpy of vaporisation of water is 40.5 kJ $m o l^{- 1}$ . Calculate the enthalpy change for the reaction :
$C H_{4 (g)} + 2 O_{2 (g)} \to C O_{2 (g)} + 2 H_{2} O_{(g)}$

Q. The normal boiling point of water is

373 K

. Vapour pressure of water at temperature 'T' is

19 m m H g

. If enthalpy of vaporisation is

40.67 k J / m o l

, then temperature 'T' would be:
(Use :

l o g 2 = 0.3, R = 8.3 J K^{- 1} m o l^{- 1})

Join BYJU'S Learning Program