At `0^(@)C` ice and water are in equilibrium and `DeltaH=6kJ" "mol^(-1)` for this process:
`H_(2)OhArrH_(2)O(l)`
The values of `DeltaS and DeltaG` for conversion of ice into liquid water at `0^(@)C` are:

At 0^@C , ice and water are in equilibrium and DeltaH = 6.0 kJ mol^(-1) for the process H_2O (s) hArr H_2O (l) What will be Delta S and DeltaG for the conversion of ice to liquid water?

At 0^(@)C , ice and water are in equilibrium and Delta H^(@) = 6.00 kJ/mol for the process H_(2)O(s) hArr H_(2)O(I) Value of Delta S^(@) for the conversion of ice to liquid water is {:((1),10.15 JK^(-1)mol^(-1),(2),17.25 JK^(-1)mol^(-1)),((3),21.98 JK^(-1)mol^(-1),(4),30.50 JK^(-1)mol^(-1)):}

At 0^(@)C , ice and water are in equilibrium and Delta H^(@) = 6.00 kJ/mol for the process H_(2)O(s) hArr H_(2)O(I) Value of Delta S^(@) for the conversion of ice to liquid water is {:((1),10.15 JK^(-1)mol^(-1),(2),17.25 JK^(-1)mol^(-1)),((3),21.98 JK^(-1)mol^(-1),(4),30.50 JK^(-1)mol^(-1)):}

At 0^(@)C ice and water are in equilibrium and Delta H= 6.0KJ " then " Delta S will be

At 0^(@)C ice and water are in equilibrium and Delta H= 6.0KJ " then " Delta S will be