CameraIcon

SearchIcon

MyQuestionIcon

3

You visited us 3 times! Enjoying our articles? Unlock Full Access!

Gibbs Free Energy & Spontaneity

Calculate the...

Question

Calculate the entropy change when 36 g of liquid water evapourates at 373 K .Change in Enthalpy of vapourisation =40.63KJ/mol

Open in App

Solution

$∆ S_{V a p} = \frac{∆ H_{V a p}}{T_{b}} = \frac{40.63 \times 1000}{373} = 109 J K^{- 1} m o l^{- 1} E n t r o p y c h a n g e f o r t h e e v a p o r a t i o n o f 36 g o f w a t e r = \frac{109}{18} \times 36 = 218 J K^{- 1}$

Suggest Corrections

thumbs-up

0

Similar questions

Q. Calculate the entropy change when

36 g

of liquid water evaporate at

373 K

(latent heat of vaporization of water is

0.63 k J m o l^{- 1}

Q. The enthalpy change, for the transition of liquid water to steam,

Δ H_{v a p o u r}

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

373 K

. Calculate the entropy change for the process.

Q. Calculate the entropy increase in the evaporation of 1 mole of a liquid when it boils at

100^{0} C

having heat of vapourisation at

100^{0} C

0^{o} C

, if enthalpy of vapourisation of ice is 40.65

k J / m o l

. the molar entropy change for melting of ice at

0^{o} C

k J / m o l

.

0^{o} C

, if enthalpy of vapourisation of ice is 40.65

k J / m o l

. the molar entropy change for melting of ice at

0^{o} C

k J / m o l

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Gibbs Free Energy

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Gibbs Free Energy & Spontaneity

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon