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Heat of Formation

Ionisation en...

Question

Ionisation energy of $A l t o A l^{3 +} = 5137 k J m o l^{- 1} △ H_{h y d r a t i o n} o f : A l^{3 +} = - 4665 k J m o l^{- 1} a n d f o r C l^{-} = - 381 k J m o l^{- 1} .$ Which of the following statement is correct?

A l C l_{3}

would remain covalent in aqueous solution

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Only at infinite dilution

A l C l_{3}

undergoes ionisation

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In aqueous solution

A l C l_{3}

becomes ionic

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None of these

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Solution

The correct option is C In aqueous solution $A l C l_{3}$ becomes ionic
If $A l C l_{3}$ is present in ionic state in aqueous solution, therefore it has $A l^{3 +} a n d 3 C l^{-}$
Standard heat of hydration of $A l^{3 +}$ and $3 C l^{-}$ ions
$= (△ H)_{h y d r a t i o n} f o r A l^{+ 3} + 3 \times (△ H)_{h y d r a t i o n} f o r C l^{-}$
$= - 4665 + 3 \times (- 381) k J m o l^{- 1}$
$= - 5808 k J / m o l$
Required energy of ionisation of $A l = 5137 k J m o l^{- 1}$
$∴$ Hydration energy dominates ionisation energy
$∴ A l C l_{3}$ would be ionic in aqueous solution.

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Similar questions

A l t o A l^{3 +} = 5137 k J m o l^{- 1} △ H_{h y d r a t i o n} o f : A l^{3 +} = - 4665 k J m o l^{- 1} a n d f o r C l^{-} = - 381 k J m o l^{- 1} .

A l t o A l^{3 +} = 5137 k J m o l^{- 1} △ H_{h y d r a t i o n} o f : A l^{3 +} = - 4665 k J m o l^{- 1} a n d f o r C l^{-} = - 381 k J m o l^{- 1} .

A l C l_{3}

= 5137 K J m o l^{- 1}

△ H h y d r a t i o n A l^{3 +} = - 4665 K J / m o l^{- 1}

△ H h y d r a t i o n C l^{-} = - 381 K J / m o l^{- 1}

A l C l_{3}

A l = 5137 k J m o l^{- 1}

Δ H

A l^{3 +} = - 4665 k J m o l^{- 1};

Δ H

C l^{-} = - 381 k J m o l^{- 1}

A l {C l}_{3}

A l {C l}_{3} = 5137

^{- 1}

Δ_{H y d r a t i o n}

{A l}^{3 +} = - 4665

^{- 1}

Δ_{H y d r a t i o n}

{C l}^{-} = - 381

^{- 1}

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