[" (c) Spontaneous and reversible "],[" 17.At "0^(@)C Delta_(" fus ")H^(@)=6kJ" mole "^(-1)" ,change of entropy for freezing "1" mole ice will be "],[[" (a) "oo," (b) "0," (c) "21.98J" mole "^(-1)K" (d) "13.6J]]

At 0^(@)C,DeltaH_(fus)^(@)=6kJ //mol , change of entropy for freezing of one mole of ice will be :

At 0^(@)C,DeltaH_(fus)^(@)=6kJ //mol , change of entropy for freezing of one mole of ice will be :

IF the melting point of ice is 273 K and molar enthalpy of usion for ice = 6.0 kJ mol^(-1) , the change in entropy for the fusion of 1 mole of ice will be

IF the melting point of ice is 273 K and molar enthalpy of usion for ice = 6.0 kJ mol^(-1) , the change in entropy for the fusion of 1 mole of ice will be

Enthalpy of fusion of water is 6.01 kJ mol^(-1) . The entropy change of 1 mole of ice at its melting point will be:

The latent heat of melting of ice at 0^(@)C is 6 kJ "mol"^(-1) . The entropy change during the melting in JK^(_1) "mol"^(-1) is closest to-

Calculate enthalpy change on freezing 1 mol water at 10^(@)C to ice at -10^(@)C. Delta_("fus")H= 6.03 " kJ mol"^(-1) " at " 0^(@)C . C_(p)[H_(2)O(l)]= 75.3 " J. mol"^(-1). K^(-1) , C_(p)[H_(2)O(s)]= 36.8 " J mol"^(-1). K^(-1) .

For a solvent Delta_(freez)H^(@)=5355" cal mole"^(-1) , molar mass is 150 and freezing point is 80^(@)C is 80^(@)C , its K_(f) will be

For a solvent Delta_(freez)H^(@)=5355" cal mole"^(-1) , molar mass is 150 and freezing point is 80^(@)C is 80^(@)C , its K_(f) will be