Home
Class 11
CHEMISTRY
Calculate the entropy changes of fustion...

Calculate the entropy changes of fustion and vaporisation for chlorine from the following data:
`Delta_(fus)H = 6.40 kJ mol^(-1)`, melting point `=- 100^(@)C`
`Delta_(vap)H = 20.4 kJ mol^(-1)`, boiling point `=- 30^(@)C`

Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the entropy changes of fusion and vapourisation for chlorine from the following data: Delta_(fus)H = 6.40 kJ mol^(-1) , melting point =- 100^(@)C Delta_(vap)H = 20.4 kJ mol^(-1) , boiling point =- 30^(@)C

Calculate entropy changes of fusion and vaporisation for chlorine from the following data : Delta_(fus) H = 6.40 kJ "mol"^(-1) m.p = -102^(@)C Delta_(vap) H = 20.4 kJ mol^(-1) b.p = - 34^(@)C

Calculate the entropy change for vaporization of 1mol of liquid water to stem at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .

Calculate the entropy change for vaporization of 1mol of liquid water to steam at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .

Calculate the enthalpy of sublimation of Na metal from the following data given Delta H_fus^@=2.6 KJ mol^(-1) Delta H_vap^@=98 KJ mol^(-1)

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 -hexane when 1mol of it evaporates at 341.7K (Delta_(vap)H^(Theta) = 290.0 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))