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The enthalpy ...

Question

The enthalpy of solution of $B a C l_{2 (s)}$ and $B a C l_{2} .2 H_{2} O_{(s)}$ are -20.6 and 8.8KJ/mol respectively. The enthalpy change for the reaction
$B a C l_{2 (s)} + 2 H_{2} O ⟶ B a C l_{2} .2 H_{2} O$

A

29.8KJ

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B

-11.8KJ

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C

-20.6KJ

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D

-29.4KJ

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Solution

The correct option is D -29.4KJ
The given reaction is

$B a C l_{2} (s) + 2 H_{2} O \to B a C l_{2} .2 H_{2} O$

Given data is;

$Δ_{r} H_{1}^{\circ} = - 20.6 k J m o l^{- 1}$

$Δ_{r} H_{2}^{\circ} = 8.8 k J m o l^{- 1}$

According to Hess’s law,

$Δ_{r} H_{1}^{\circ} = Δ_{r} H^{\circ} + Δ_{r} H_{2}^{\circ}$

$Δ_{r} H^{\circ} = - 20.6 - 8.8$
$Δ_{r} H^{\circ} = - 29.4 k J m o l^{- 1}$

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