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The enthalpy ...

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The enthalpy of formation of NaCl can be calculated by using

A

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B

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C

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D

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Similar questions

Q. During the formation of

N a C l

, which of the enthalpies are negative?

How much lattice enthalpy is released in formation of NaCl

Q. According to Born-Haber's cycle, the enthalpy of formation of ionic compounds can be determined. The formation of NaCl involves following steps –
(i)

N a (s) S - ------------ \to Energy of subtimation N a (g)

N a (g) I - ---------- \to Ionisation potenital N a^{+} (g) + e^{-}

C l_{2} (g) D - -------------- \to Bond dissociation energy 2 C l (g)

C l (g) + e^{-} E - --------- \to Electron - affinity C l^{-} (g)

C l^{-} (g) + N a^{+} (g) U - ------- \to Lattice energy N a C l (s)

The enthalpy of formation of NaCl will be -

Q. The lattice energy of

N a C l (s)

- 790 k J . {m o l}^{- 1}

and enthalpy of hydration is

- 785 k J . {m o l}^{- 1}

. Calculate the enthalpy of the solution of

N a C l (s)

.

Q. Assuming enthalpy of combustion of hydrogen at

273 K

- 286 k J

and enthalpy of fusion of ice at the same temperature to be

+ 6.0 k J

, calculate enthalpy change during formation of

100 g

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