The entropy change when `36g` of water evaporates at `373 K` is `:-` `(DeltaH=40.63(KJ)/(mol))`

Calculate the entropy change of n-hexane when 1 mole of it evaporates at 341.7 K (Delta_(vap) H = 29.0 kJ "mol"^(-1)) .

Calculate the entropy change of n -hexae when 1mol of it evaporates at 341.7K (Delta_(vap)H^(Theta) = 290.0 kJ mol^(-1))

Calculate the entropy change of n -hexane when 1mol of it evaporates at 341.7K (Delta_(vap)H^(Theta) = 290.0 kJ mol^(-1))

Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K. The molar heat of vaporization of ethanol is 39.84 kJ "mol"^(-1)

Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K. The molar heat of vapourisation of ethanol is 39.84 "kJ mol"^(-1)

Calculate the entropy change when one mole of water at 373 K is converted into steam. Latent heat of vaporisation of water (DeltaH_(v)) is 40.7 xx 10^(3) J mol^(-1)

Calculate the entropy change when one mole of water at 373 K is converted into steam. Latent heat of vaporisation of water (DeltaH_(v)) is 40.7 xx 10^(3) J mol^(-1)

Calculate the entropy change when 3.6g of liquid water is completely converted into vapour at 100^(@)C . The molar heat of vaporization is 40.85KJ mol^(-1) .