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 mol of ice. The melting point of ice is 273 K and molar enthalpy of fusion of ice = 6KJmol^(-1)

Calculate the change in entropy for the fusion of 1 mol of ice. The melting point of ice is 300K and molar enthalpy of fustion for ice = 6.0 k J mol^(-1) .

Calculate the change in entropy for the fusion of 1 mol of ice. The melting point of ice is 300K and molar enthalpy of fustion for ice = 6.0 k J mol^(-1) .

(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):}

Calculatte the molal elevation constant of water if molar enthalpy of vapourisation of water at 373K is 40.585 kJ mol^(-1) .

Calculate the entropy change during the melting of one mole of ice into water at 0^@C and 1 atm pressure. Enthalpy of fusion of ice is 6008 "J mol"^(-1) .