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

(i) Calculate the change in entropy for the fusion of 1 mole of ice. The melting point of ice is 273 K and molar enthalpy of fusion for ice = 6.0 kJ/mole. (ii) Calculate the standard of entropy change for the following reaction. {:(,H^(+)(aq), + OH(aq)to, H_(2)O(l)),(S^(@)(298 K)//JK^(-1)mol^(-1),0,-10.7,+70):}

(i) Calculate the change in entropy for the fusion of 1 mole of ice. The melting point of ice is 273 K and molar enthalpy of fusion for ice = 6.0 kJ/mole. (ii) Calculate the standard of entropy change for the following reaction. {:(,H^(+)(aq), + OH(aq)to, H_(2)O(l)),(S^(@)(298 K)//JK^(-1)mol^(-1),0,-10.7,+70):}

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:

Latent heat of fusion of ice is 6kJ mol^(-1) . Calculate the entropy change in the fusion of ice.

Latent heat of fusion of ice is 6 kJ mol^(-1) . Calculate the entropy change in the fusion of ice.

At STP if latent heat of fusion of ice is 6 kJ * mol^(-1) , then find out the entropy change of fusion of ice .

The molar enthlpy of fusion of water is 6.01KJ mol^(-1) . The entropy change of 1 mol of water at its melting point will be

Latent heat of fusion of ice is 0.333 kJ g^(-1) . The increase in entropy when 1 mole water melts at 0^(@)C will be

Latent heat of fusion of ice is 0.333 kJ g^(-1) . The increase in entropy when 1 mole water melts at 0^(@)C will be