What is the entropy change for dissolving 1 mole of NaCl at 298 K lattice energy =`+777.8KJ mol^(-1) Delta H_(Hydration) of NaCl=-774.1KJ mol^(-1), DeltaG_(dissolution) of NaCl=-914 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 enthalpy change on freezing of 1.0 mole of water at 10^@C to ice at -10^@C,triangle_(fus)H = 6.03 kJ mol^-1 at 0^@C , C_p[H_2O(l)] = 75.3 J mol^-1 K^-1 C_p[H_2O(s)] = 36.8 J mol^-1 K^-1

The enthalpy change for the transition of liquid water to steam is 40.8KJ mol^(-1) at 373 K calculate the entropy of evaporation of water.

Determine the standard enthalpy of formation of isoprene(g) at 298K temperature. Given: at 298K, DeltaH^(0)(C-H)=413kJ*mol^(-1) DeltaH^(0)(H-H)=436kJ*mol^(-1) DeltaH^(0)(C-C)=346kJ*mol^(-1) , DeltaH^(0)(C=C)=611kJ*mol^(-1) , C("graphite, s")toC("graphite, g"), DeltaH^(0)=717kJ*mol^(-1)

Calculate the entropy change in the surrounding when 1,00 mol of H_(2)O(l) is formed under standard conditions. Delta_(f)H^(0)=-286kJ*mol^(-1)

Draw the Born-Haber cycle for the formation of LiF(s) from its elements and using this cycle calculate the lattice enthalpy of LiF(s). Given: DeltaH_(f)^(0)[LiF(s)]=-617kJ*mol^(-1) , DeltaH_(sub)=+161kJ*mol^(-1),DeltaH^(0)(F-F)=+159kJ*moL^(-1) , IE_(1)=+520kJ*mol^(-1),EA of F=-328kJ*mol^(-1) .

Calculate the entropy change in surroundings when 1.00 mole of H_2O(l) is formed under standard conditions. triangle_fH^@ = 286 kJ mol^-1 .

Calculate the free energy change and entropy change per mole when liquid water boils at 1 atmosphere latent heat of vaporization of water= 2.0723KJ mol^(-1)

Calculate the value of standard reaction enthalpy for the following reaction : C_2H_5Cl (g) rarr C_2H_4 (g) + HCl (g) at 298 K temperature.Given that DeltaH^@ (C-H) = 413 KJ mol^-1, DeltaH^@ (C-C) = 346 KJ mol^-1 ,DeltaH^@ (C=H) =611 KJ mol^-1, DeltaH^@ (C-CI) = 339 KJ mol^-1 DeltaH^@ (H-Cl) = 432 KJ- mol^-1 .

If the enthalpy change for the transition of liquid water to steam is 30kJ*mol^(-1) at 27^(@)C , the entropy change in J*mol^(-1)*K^(-1) for the process would be-