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 "Mole"^(-1)

Calculate the entropy change during the melting of one mole of ice int

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 "Mole"^(-1)
Answer» `22.007 "J K"^(-1) "MOLE"^(-1)` 22.007 J K Mole `220.07 "J K"^(-1) "Mole"^(-1)` `2.2007 "J K"^(-1)` Mole Solution :Enthalpy of fusion of ice = 6008 J `"MOL"^(-1) =DeltaH` `DELTAS=(DeltaH)/T_m "" T_m =0^@C` = 273 K Entropy of fusion = `"Enthalpy of fusion of ice "/"Melting point (Kelvin)"` `DeltaS=6008/273 =22.007 J K^(-1) "mol"^(-1)`