Calculated the Gibbs energy change on dissolving one mole of sodium chloride at `25^(@)C`.
Lattice `=+ 777.0 kJ mol^(-1)`
Hydration of `NaCI =- 774.0 kJ mol^(-1)`
`DeltaS` at `25^(@)C = 40 J K^(-1) mol^(-1)`

Calculate the Gibbs energy change on dissolving one mole of sodium chloride at 25^(@)C . Lattice energy = + 777.8 kJ "mol"^(-1) Hydration of NaCI = -774.1 kJ "mol"^(-1) DeltaS at 25^(@)C = 43 JK^(-1) "mol"^(-1) .

Calculate the free energy change when one mole of sodium chloride is dissolved in water at 298 K. (Given : Lattice energy of NaCl = - 777.8 kJ mol^(-1) , Hydration energy of NaCl = 774.1 kJ mol^(-1) and DeltaS " at" 298 K = 0.043 kJ mol^(-1) .

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 free energy change when 1 mole of NaCl is dissolved in water at 298 K. (Given : Lattice energy of NaCl = -777.8 kJ mol^(-1) ), Hydration energy -774.1 kJ mol^(-1) and Delta S = 0.043 kJ mol^(-1) mol^(-1) at 298 K).

What is the free energy change in dissolving one mole of NaCl with its lattice energy and hydration energy of -777.8 kJ mol^-1 and -774 kJ mol^-1 respectively at 25^@ C ? (Given: DeltaS=0.043 kJ K^-1 mol^-1 )

Calculate the free enegry change when 1mol of NaCI is dissolved in water at 298K . Given: a. Lattice enegry of NaCI =- 778 kJ mol^(-1) b. Hydration energy of NaCI - 774.1 kJ mol^(-1) c. Entropy change at 298 K = 43 J mol^(-1)

Calculate the free enegry change when 1mol of NaCI is dissolved in water at 298K . Given: a. Lattice enegry of NaCI =- 778 kJ mol^(-1) b. Hydration energy of NaCI - 774.3 kJ mol^(-1) c. Entropy change at 298 K = 43 J mol^(-1)