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Calculated the Gibbs energy change on di...

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)`

Text Solution

AI Generated Solution

To calculate the Gibbs energy change (ΔG) on dissolving one mole of sodium chloride (NaCl) at 25°C, we will follow these steps: ### Step 1: Convert Temperature to Kelvin The temperature given is 25°C. To convert this to Kelvin, we use the formula: \[ T(K) = T(°C) + 273 \] So, \[ T = 25 + 273 = 298 \, K \] ...
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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) .

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)

Knowledge Check

  • The enthalpy of solution of sodium chloride is 4 kJ mol^(-1) and its enthalpy of hydration of ion is -784 kJ mol^(-1) . Then the lattice enthalpy of NaCl (in kJ mol^(-1) ) is

    A
    a. `+"780 kJ mol"^(-1)`
    B
    b. `+"394 kJ mol"^(-1)`
    C
    c. `+"788 kJ mol"^(-1)`
    D
    d. `+"398 kJ mol"^(-1)`

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