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

State giving reasons whether the entropy change for vaporisation of one mole of water will be more or less than entropy change per mole for fusion of ice.

Enthalpy change for the process, H_(2)O"(ice")hArr H_(2)O"(water)" is "6.01 kJ mol"^(-1) . The entropy change of 1 mole of ice at its melting point will be

Enthalpy change for the process, H_(2)O"(ice")hArr H_(2)O"(water)" is "6.01 kJ mol"^(-1) . The entropy change of 1 mole of ice at its melting point 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:

Calculate the change in entropy for the fusion of 1 mole of ice (water). The melting point of water is 273 K and molar enthalpy of funsion for water =6.0 kJ mol^(-1)

Calculate the change in entropy for the fusion of 1 mole of ice (water). The melting point of water is 273 K and molar enthalpy of funsion for water =6.0 kJ mol^(-1)