For the process, `H_(2)O(l) to H_(2)O(g)`

Entropy changes for the process H_(2)O(l) rarr H_(2)O(g) at normal pressure and 274 K are given below Delta G_(system) = - 22.13, Delta S_("surroundings") = + 22.05 Then process is non spontaneous because

For the process, H_2O(l) rarr H_2O_((g)) at 100^@C, DeltaS is

Which of the followingk is true for the process H_(2) O (s) = H_(2) O (l) at 0^(@)C and 1 atm?

At 25^(@)C, Delta G^(0) for the process H_(2)O_((l)) hArr H_(2) O_((g)) is 8.6kJ. The vapour pressure of water at this temperature, is nearly

For a process H_(2)O(s) rarr H_(2)O(l) at 273 K

For a process H_(2)O(s) rarr H_(2)O(l) at 273 K

Calculate the enthalpy of vaporisation for water form the following: H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(g),DeltaH =- 57.0 kcal H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(l),DeltaH =- 68.3 kcal Also calculate the heat required to change 1g H_(2)O(l) to H_(2)O(g)

Calculate the enthalpy of vaporisation for water form the following: H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(g),DeltaH =- 57.0 kcal H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(l),DeltaH =- 68.3 kcal Also calculate the heat required to change 1g H_(2)O(l) to H_(2)O(g)