Find the heat change in the reaction NH3g - HCl g - NH4 Cls from the following data NH3 g - aq - NH3 aq- - H - - 8-4 K- Cal- HClg - aq - HClaq- - H - -17-3 K- Cal- NH3aq - HClaq - NH4 Claq- - H - - 12-5 K- Cals- NH4 Cls - aq - NH4 Claq- - H - - 3-9 K- Cal-

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Thermodynamic Processes

Find the heat...

Question

Find the heat change in the reaction
$N H_{3} (g) + H C l (g) \to N H_{4} C l (s)$ from the following data
$N H_{3} (g) + a q \to N H_{3} (a q),$ $Δ H = - 8.4 K . C a l .$
$H C l (g) + a q \to H C l (a q),$ $Δ H = - 17.3 K . C a l .$
$N H_{3} (a q) + H C l (a q) \to N H_{4} C l (a q), Δ H = - 12.5 K . C a l s .$
$N H_{4} C l (s) + a q \to N H_{4} C l (a q), Δ H = + 3.9 K . C a l .$

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Solution

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$N H_{4} C l (s) + H_{2} O \to N H_{4} C l (a q);$ $Δ H = 16.3 k J$ .

In the above reaction, $Δ H$ represents:

Δ H_{f}^{o}

\frac{1}{2} H_{2} (g) + \frac{1}{2} C l_{2} (g) \to H C l (g)

Δ H = - 92.4

H C l (g) + N H_{2} O

\to H^{+} (a q) + C l^{-} (a q)

Δ H = - 74.8

Δ H_{f}^{o} (H^{+} (a q)) = 0.0

{Δ H}_{f}^{o}

\frac{1}{2} H_{2} (g) + \frac{1}{2} {C l}_{2} (g ⟶ H C l (g); Δ H = - 92.4 k J {m o l}^{- 1}

H C l (g) + n H_{2} O ⟶ H^{+} (a q .) + {C l}^{-} (a q .); Δ H = - 74.8 k J {m o l}^{- 1}

Δ H_{f (H^{+} (a q .)}^{o} = 0.0 k J {m o l}^{- 1}

{A l}_{2} {C l}_{6}

2 A l (s) + 6 H C l (a q) ⟶ {A l}_{2} {C l}_{6} (a q) + 3 H_{2} (g), Δ H = - 239.76 k c a l

H_{2} (g) + {C l}_{2} (g) ⟶ 2 H C l (g); Δ H = - 44.0 k c a l

H C l (g) + A q ⟶ H C l (a q); Δ H = - 17.32 k c a l

{A l}_{2} {C l}_{6} (s) + A q ⟶ {A l}_{2} {C l}_{6} (a q); Δ H = - 153.69 k c a l

A g^{+} (a q) + C l^{-} (a q) \to A g C l (s)

N H_{4} C l (s) \to N H_{3} (g) + H C l (g)

2 N H_{3} (g) \to N_{2} (g) + 3 H_{2} (g)

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