Home
Class 11
CHEMISTRY
Calculate the entropy change of n-hexae ...

Calculate the entropy change of `n`-hexae when `1mol` of it evaporates at `341.7K (Delta_(vap)H^(Theta) = 290.0 kJ mol^(-1))`

Text Solution

Verified by Experts

`Delta_(vap)S = (Delta_(vap)H)/(T_(b)) = (29.0 xx 10^(3))/(341.7) = 84.87 J K^(-1) mol^(-1)`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Ex 6.5|30 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Exercises (Subjective)|70 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Ex 6.3|27 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

Calculate the entropy change of n-hexane when 1 mole of it evaporates at 341.7 K (Delta_(vap) H = 29.0 kJ "mol"^(-1)) .

Calculate the entropy change for vaporization of 1mol of liquid water to stem at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .

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

A swimmer coming out from a pool is covered with a film of water weighing about 18 g. how much heat must be supplied to evaporate this water at 298 K ? Calculate the internal energy of vaperization at 100^(@)C . Delta_(vap)H^(Theta) for water at 373 K = 40.66 kJ mol^(-1)

Calculate the entropy change for a reaction: XrarrY Given that DeltaH^(Theta) = 28.40 kJ mol^(-1) and equilibrium constant is 1.8 xx 10^(-7) at 298K .

Calculate the temperature at which liquid water will be in equilibrium with water vapour. Delta_(vap)H = 40.00 kJ mol^(-1) and Delta_(vap)S = 0.100 kJ mol^(-1)K^(-1)