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  • The lattice energy of solid NaCl is 200 Kcal/mol. The enthalpy of dissolution of solid NaCl is endothermic to the extent of 1Kcal/mol. If the hydration enthalpy of <im

The lattice energy of solid NaCl is 200 Kcal/mol. The enthalpy of dissolution of solid NaCl is endothermic to the extent of 1Kcal/mol. If the hydration enthalpy of \mathrm{ Na^+} and \small \mathrm{Cl^-} are in the ratio of 7:6, then what is the enthalpy of hydration (in Kcal/mol) of sodium ions?

Option: 1

107


Option: 2

-107


Option: 3

-199


Option: 4

-92


Answers (1)

best_answer

As we learnt,

Enthalpy of Solution = Lattice Energy + Hydration Enthalpy

\mathrm{\Delta _{sol}H=\Delta _{lattice}H+\Delta _{hyd}H}

Or we can also write it as,

\mathrm{1=200 + \Delta _{hyd}H}

\Rightarrow \mathrm{\Delta _{hyd}H=-199\ kcal\ mol^-}

It is given that ratio of hydration enthalpies of Na+ and Cl- ions is 7:6

 

Hydration energy of Na+ ions = \frac{7}{7+6}\times (-199) =  -107 Kcal/mol

 

 

Posted by

manish painkra

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