Calculate the entropy change in JK-1 mol -1 for vaporisation of liquid water to steam at 100- C- Given that heat of vaporisation is 40-8 kJ mol-1-

We know that, Δ S=Δ H_vT Here given that, Δ H=40.8 kJ/mol, T=373K putting the values, Δ S=40.8×10^3373=109.38 JK^ 1mol^ 1 Theory: Entropy Calculation with ...

You visited us 6 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XIII

Chemistry

Entropy

Calculate the...

Question

Calculate the entropy change (in $J K^{- 1} m o l^{- 1}$ ) for vaporisation of liquid water to steam at $100^{\circ} C$ . Given that heat of vaporisation is $40.8 k J m o l^{- 1}$ .

109.38

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

100.38

No worries! We‘ve got your back. Try BYJU‘S free classes today!

120.38

No worries! We‘ve got your back. Try BYJU‘S free classes today!

129.38

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A 109.38
We know that,
$Δ S = \frac{Δ H_{v}}{T}$
Here given that,
$Δ H = 40.8 k J / m o l, T = 373 K$
putting the values,
$Δ S = \frac{40.8 \times 10^{3}}{373} = 109.38 J K^{- 1} {mol}^{- 1}$

Theory:

Entropy Calculation with phase transformation:
Phase change occurs at constant Pressure & Temperature and is considered reversible if it occurs at its transition temperature.

Entropy change for Vaporisation:
At constant pressure $q = q_{p}$ = $Δ H$
$Δ S_{v a p}$ = $\frac{Δ H_{v a p}}{T_{b}}$ where $T_{b}$ is boiling point of a substance.

Suggest Corrections

Similar questions

Q. Calculate the entropy change (in

J K^{- 1} m o l^{- 1}

) for vaporisation of liquid water to steam at

100^{\circ} C

. Given that heat of vaporisation is

40.8 k J m o l^{- 1}

Q. The entropy change for vaporisation of water to steam at

100^{o}

C in

{J K}^{- 1} {m o l}^{- 1}

is :

[Given that the heat of vaporisation is

{40.8 k J m o l}^{- 1}

Q. Calculate the entropy change (in

J K^{- 1} m o l^{- 1}

) for vaporisation of liquid water to steam at

100^{\circ} C

. Given that heat of vaporisation is

40.8 k J m o l^{- 1}

Q. The entropy change for vaporisation of a liquid is

109.3 j K^{- 1} m o l^{- 1}

. The molar heat of vaporistion of that liquid is

40.77 k J m o l^{- 1}

. Calculate the boiling points of that liquid.

Q. Latent heat of vaporisation of water is

540 c a l g^{- 1}

100^{o} C

. Calculate the entropy change when

1000 g

water is converted to steam at

100^{o} C

Join BYJU'S Learning Program

Explore more

Entropy

Standard XIII Chemistry

Join BYJU'S Learning Program

Calculate the entropy change (in JK−1 mol −1) for vaporisation of liquid water to steam at 100∘C. Given that heat of vaporisation is 40.8 kJmol−1.

Calculate the entropy change (in $J K^{- 1} m o l^{- 1}$ ) for vaporisation of liquid water to steam at $100^{\circ} C$ . Given that heat of vaporisation is $40.8 k J m o l^{- 1}$ .