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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

Verified by Experts

`DeltaH =` Lattice energy - Hydration enegry
`=777 - 774 = 3kJ mol^(-1)`
`DeltaG = DeltaH - T DeltaS = 3 - 298 (40 xx 10^(-3))`
`=- 392 kJ mol^(-1)`
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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 in dissolving one mole of sodium chloride at 25^(@)C . Lattic energy = + 777.8 kJ mol^(-1) . Hydration energy of NaCl = - 774.1 kJ mol^(-1) and Delta S at 25^(@)C = 0.0 43kJ K^(-1) mol^(-1)

Knowledge Check

  • 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 )

    A
    `-18.2 kJ mol^-1`
    B
    `-36.4 kJ mol^-1`
    C
    `-9.1 kJ mol^-1`
    D
    `18.2 kJ mol^-1`

  • Calculate the Gibb's energy change when 1 mole of NaCI is dissolved in water at 25^(@)C . Littice energy of NaCI=777.8 KJ mol^(-1),DeltaS for dissolution = 0.043 KJ mol^(-1) and hydration energy of NaCI=-774.1 KJ mol^(-1) -

    A
    `-9.114 KJ mol^(-1)`
    B
    `-11.4 KJ mol^(-1)`
    C
    `-5.2 KJ mol^(-1)`
    D
    `-4.5 KJ mol^(-1)`

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

    A
    `+ 788`
    B
    `+4`
    C
    `+398`
    D
    `+780`

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    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)

    Calculate the entropy change for vaporization of 1mol of liquid water to stem at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .

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