.What is lattice energy entropy

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Solution

Lattice enthalpy Î”H_LE(compound) is defined as the energy released when 1 mole of a solid is formed from its separated gaseous ions.

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Calculate the free energy change when 1 mol of NaCl is dissolved in water at 298 K. given:
(i) Lattice energy of NaCl = -778 kJ $m o l^{- 1}$
(ii) Hydration energy of NaCl = -778 kJ $m o l^{- 1}$
(iii) Entropy change at 298 K = 43 J $m o l^{- 1}$

Q. If the Gibbs free energy change when 1 mole of

N a C l

is dissolved in water at 298K is

x

kJ, then -

1000 x

is
Given that,
(a) Lattice energy of

N a C l

778 k J {m o l}^{- 1}

(b) Hydration energy of

N a C l = - 774.3 k J {m o l}^{- 1}

298 K = 43 J {m o l}^{- 1}

Q. What is lattice energy

Q. The free energy change when 1 mole of

N a C l

is dissolved in water at 298 K is

- x k J

. Find the value of 'x'.
Given:-

Lattice energy of N a C l = 778 k J m o l^{- 1}

Hydration energy of N a C l = - 775 k J m o l^{- 1}

Entropy change (at 298 K) = 40 J m o l^{- 1}

What is meant by Lattice energy, ionisation energy.

Sir/Ma'am what is the difference between them

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.What is lattice energy entropy

Lattice enthalpy Î”HLE(compound) is defined as the energy released when 1 mole of a solid is formed from its separated gaseous ions.

Lattice enthalpy Î”H_LE(compound) is defined as the energy released when 1 mole of a solid is formed from its separated gaseous ions.