Home
Class 12
CHEMISTRY
For vaporization of water at 1 atmospher...

For vaporization of water at 1 atmospheric pressure, the values of `DeltaH and DeltaS` are `40.63 "kJ mol"^(-1) and 108.8 "JK"^(-1) mol^(-1)` respectively. The temperature when Gibbs energy change `(DeltaG)` for this transformation will be zero , is :

Text Solution

Verified by Experts

The correct Answer is:
373.4
`H_(2)O(l) overset(1 atm) `DeltaH = 406.30 J mol^(-1)`
`DeltaS = 108.8 JK^(-1) mol^(-1)`
`DeltaG = DeltaH - T DeltaS`
When `DeltaG =0`,
`DeltaH -TDeltaS=0`
`T = (DeltaH)/(DeltaS) = (40630 J "mol"^(-1))/(108.8 J "mol"^(-1)) = 373.4` K
Promotional Banner

Topper's Solved these Questions

  • CHAPTERWISE NUMERIC/INTEGER ANSWER QUESTIONS

    DISHA PUBLICATION|Exercise Chapter-7: EQUILIBRIUM|15 Videos

  • CHAPTERWISE NUMERIC/INTEGER ANSWER QUESTIONS

    DISHA PUBLICATION|Exercise CHAPTER-8: REDOX REACTIONS|15 Videos

  • CHAPTERWISE NUMERIC/INTEGER ANSWER QUESTIONS

    DISHA PUBLICATION|Exercise Chapter-5: STATES OF MATTER|15 Videos

  • BIOMOLECULES

    DISHA PUBLICATION|Exercise Exercise - 2 : Concept Applicator|30 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    DISHA PUBLICATION|Exercise EXERCISE-2: CONCEPT APPLICATOR|30 Videos

Similar Questions

Explore conceptually related problems

For vaporization of water at 1 atmospheric pressure the values of Delta H and Delta S are 50.63 kJ mol^9-1) and 118.8 JK ^(-1) mol^(-1) respectively. The temperature when Gibbs energy change (Delta G) for this transformation will be zero, is

For vaporization of water at 1 atmospheric pressure the values of DeltaH and DeltaS are 40.63KJmol^(-1) and 108JK^(-1)mol^(-1) , respectively. The temperature when Gibbs energy change (DeltaG) for this transformation will be zero is

For a certain reaction X rarr Y the value of DeltaH and DeltaS are 50.50KJ mol^(-1) and 100.03JK^(-1) respectively. The temperature at which DeltaG=0 is

For the reaction, Ag_(2)O(s)hArr2Ag(s)+(1)/(2)O_(2)(g) DeltaH,DeltaS and T are 40.63 kJ mol^(-1) , 108.8 JK^(-1)mol^(-1) and 373.4K respectively. Free energy change DeltaG of the reaction will be:

The values of DeltaH and Delta S of a certain reaction are -400 kJ mol^-1 and -20 kJ mol^-1 K^-1 respectively. The temperature below which the reaction is spontaneous is _________.

The value of DeltaH and DeltaS for a reaction are respectively 30 kJ mol^(-1) and 100JK^(-1)mol^(-1) . Then temperature above which the reaction will become spontaneous is:

DeltaH and DeltaS for the system H_2O_((l))hArr H_2O_((g)) at 1atm are 40.63 kJ mol^(-1) and 108.8 JK^(-1) mol^(-1) respectively. The temperature at which the rates of forward and backward reactions will be same: