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The enthalpy of solution of sodium chlor...

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

Text Solution

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`+ 788kJ mol^(-1)( Delta_("sol") H = Delta_("lattice")H + Delta_(hyd) H ) `
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Knowledge Check

  • 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`

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

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

  • The standard enthalpy of formation of NH_(3) is -46.0 kJ mol^(-1) . If the enthalpy of formation of H_(2) from its atoms is -436 kJ mol^(-1) and that of N_(2) is -7112kJ mol^(-1) , the average bond enthalpy of N-H bond in NH_(3) is :-

    A
    `-1102 kJ mol^(-1)`
    B
    `-964 kJ mol^(-1)`
    C
    `+352 kJ mol^(-1)`
    D
    `+1056 kJ mol^(-1)`

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