Home
Class 12
CHEMISTRY
Calculate the entropy change when one mo...

Calculate the entropy change when one mole of water at 373 K is converted into steam. Latent heat of vaporisation of water `(DeltaH_(v))` is `40.7 xx 10^(3) J mol^(-1)`

Text Solution

AI Generated Solution

To calculate the entropy change when one mole of water at 373 K is converted into steam, we can use the formula for entropy change (\( \Delta S \)) during a phase transition: \[ \Delta S = \frac{\Delta H}{T} \] Where: - \( \Delta S \) = change in entropy ...
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the entropy change (DeltaS) when 1 mol of ice at 0^(@)C is converted into water at 0^(@)C . Heat of fusion of ice at 0^(@)C is 1436 cal per mol.

Calculate the entropy change when 3.6g of liquid water is completely converted into vapour at 100^(@)C . The molar heat of vaporization is 40.85KJ mol^(-1) .

Entropy change involve in conversation of 1 mole of liquid water at 373K to vapour at the same temperature (latent heat of vaporisation of water= 2.257kJg^(-1))

Calculate the entropy change for vapourisation of water if latent heat of vapourisation for water is 540 cal/g. ( K_(b) for water =0.51 K. kg "mole"^(-1) )

Calculate the entropy change for vaporization of water if latent heat of vaporization for water is 2.26 kJ/gram. The K_(b) for H_(2)O is 0.51 K/molality

Calculate the entropy change when 20.0 g of ice changes to liquid water at 0°C. The heat of fusion is 80.0 cal g^(-1) .

ΔHvap for water is 40.7 KJ mol^(−1) . The entropy of vaporization of water is:

What is Delta U when 2.0 mole of liquid water vaporises at 100^(@)C ? The heat of vaporisation (Delta H_("vap".)) of water at 100^(@)C is 40.66 KJmol^(-1) .

A thermally isolated vessel contains 100g of water at 0^(@)C . When air above the water is pumped out, some of the water freezes and some evaporates at 0^(@)C itself. Calculate the mass of the ice formed such that no water is left in the vessel. Latent heat of vaporization of water at 0^(@)C=2.10xx10^(6)J//kg and latent heat of fusion of ice =3.36xx10^(5)J//kg .

The entropy change when 36g of water evaporates at 373 K is :- (DeltaH=40.63(KJ)/(mol))