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Heat of Reaction

The value of ...

Question

The value of $Δ H_{s o l .}$ of $B a C l_{2} (s)$ and $B a C l_{2} . 2 H_{2} O (s)$ are - a kJ and b kJ respectively. The value of $Δ H_{H y d r a t i o n}$ of $B a C l_{2} (s)$ is:

A

b - a

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B

a + b

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C

- a - b

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D

a - b

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Solution

The correct option is D - a - b
Solution:- (C) $- a - b$
${B a {C l}_{2}}_{(s)} + a q . ⟶ {B a {C l}_{2}}_{a q .} Δ H = - a k J . . . . . (1)$
${B a {C l}_{2} .2 H_{2} O}_{(s)} + a q . ⟶ {B a {C l}_{2}}_{(a q .)} + 2 H_{2} O Δ H = b k J$
${B a {C l}_{2}}_{(a q .)} + 2 H_{2} O ⟶ {B a {C l}_{2} .2 H_{2} O}_{(s)} + a q . Δ H = - b k J . . . . . (2)$
Adding ${e q}^{n} (1) & (2)$ , we have
${B a {C l}_{2}}_{(s)} + a q . + {B a {C l}_{2}}_{(a q .)} + 2 {H_{2} O}_{(l)} ⟶ {B a {C l}_{2}}_{a q .} + {B a {C l}_{2} .2 H_{2} O}_{(s)} + a q . Δ H = (- a) + (- b)$
${B a {C l}_{2}}_{(s)} + 2 {H_{2} O}_{(l)} ⟶ B a {C l}_{2} .2 H_{2} O Δ H = - a - b k J$
Hence the heat of hydration of anhydrous $B a {C l}_{2}$ is $- a - b k J$ .

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