At `0^(@)C` , ice and water are in reuilibrium and `DeltaS` and `DeltaG` for the conversion of ice to liquid water is

At 0^(@)C , ice and water are in equilibrium and DeltaS and DeltaG for the conversion of ice to liquid water is,if Delta H = 7kJmol^-1

At 0^(@)C , ice and water are in equilibrium and DeltaG and DeltaS for the conversion of ice to liquid water is,if Delta H=6J 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

The conversion of water into ice is and

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?

What is the entropy change (in JK^(-1) mol^(-1)) when one mole of ice is converted into water at 0^(@)C ? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol^(-1) at 0^(@)C )