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The dissoluti...

Question

The dissolution of $C a C l_{2} \cdot 6 H_{2} O$ in a large volume of water is endothermic to the extent of $3.5 K c a l m o l^{- 1}$ . For the reaction, $C a C l_{2} (s) + 6 H_{2} O (l) ⟶ C a C l_{2} \cdot 6 H_{2} O (s)$
$Δ H$ is $- 23.2 K c a l$ . The heat of solution of anhydrous $C a C l_{2}$ in large quantity of water will be:

A

Δ H = - 16.7 K c a l m o l^{- 1}

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B

Δ H = - 19.7 K c a l m o l^{- 1}

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C

Δ H = 19.7 K c a l m o l^{- 1}

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D

.

Δ H = 16.7 K c a l m o l^{- 1}

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Solution

The correct option is C $Δ H = - 19.7 K c a l m o l^{- 1}$
$Δ H = Δ H_{1} +$ $Δ H_{2} = - 23.2 + 3.5 = - 19.7 K c a l / m o l$

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Similar questions

Following are the thermochemical reactions:

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 68.39

K + H_{2} O \to K O H (a q) + \frac{1}{2} H_{2}; Δ H = - 48.0

K O H + H_{2} O \to K O H (a q); Δ H = - 14.0

The heat of formation (in kcal/mol) of

K O H

C (s) + O_{2} (g) \to C O_{2}, (g);

Δ H = - 94.3

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g);

Δ H = - 67.4

O_{2} (g) \to 2 O (g);

Δ H = 117.4

C O (g) \to C (g) + O (g);

Δ H = 230.6

kcal/mol.
Calculate

Δ H

C (s) \to C (g)

C s O H + H C l ⟶ C s C l + H_{2} O; Δ H = - 13.4 K c a l m o l^{- 1} . . . . (i)

C s O H + H F ⟶ C s F + H_{2} O; Δ H = - 16.4 K c a l m o l^{- 1} . . . . (i i)

Δ H

for the ionisation of

H F

H_{2} O

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94.3

C O (g) + 1 / 2 O_{2} (g) \to C O_{2} (g); Δ H = - 67.4

O_{2} (g) \to 2 O (g); Δ H = 117.4

C O (g) \to C (g) + O (g); Δ H = 230.6

Δ H

C (s)

\to

C (g)

Q. What is the value of

Δ H

for the reaction

X + 2 Y \to 2 Z

?

W + X \to 2 Y

Δ H = - 400

2 W + 3 X \to 2 Z + 2 Y

Δ H = - 150

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