Calculate the heat formation of anhydrous - Al - 2 Cl - 6- from- 2Al-s-6HCl-aq- Al - 2 Cl - 6 -aq-3 H - 2 -g- H-239-76kcal- H - 2 -g- Cl - 2 -g- 2HCl-g- H-44-0kcal- HCl-g-Aq- HCl-aq- H-17-32kcal- Al - 2 Cl - 6 -s-Aq- Al - 2 Cl - 6 -aq- H-153-69kcal-

2Al( s ) + 3Cl _ 2 ( s ) ⟶ Al _ 2 Cl _ 6 ( s ) Δ H=? (i) #160; 2Al( s ) +6HCl( aq ) → Al _ 2 Cl _ 6 ( aq ) +3 H _ 2 ( or ) , Δ H _ 1 = 239.76k ...

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Heat of Formation

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Question

Calculate the heat formation of anhydrous ${A l}_{2} {C l}_{6}$ from
$2 A l (s) + 6 H C l (a q) ⟶ {A l}_{2} {C l}_{6} (a q) + 3 H_{2} (g), Δ H = - 239.76 k c a l$
$H_{2} (g) + {C l}_{2} (g) ⟶ 2 H C l (g); Δ H = - 44.0 k c a l$
$H C l (g) + A q ⟶ H C l (a q); Δ H = - 17.32 k c a l$
${A l}_{2} {C l}_{6} (s) + A q ⟶ {A l}_{2} {C l}_{6} (a q); Δ H = - 153.69 k c a l$

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A l_{2} C l_{2}

2 A l (s) + 6 H C l (a q) \to A l_{2} C l_{6} (a q) + 3 H_{2} (g), △ H = - 239.76 k c a l

H_{2} (g) + C l_{2} (g) \to 2 H C l (g), △ H = - 44.0 k c a l

H C l (g) + A q \to H C l (a q), △ H = - 17.32 k c a l

A l_{2} C l_{6} (s) + A q \to A l_{2} C l_{6} (a q), △ H = - 153.69 k c a l

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} + 1004.2 k J

H_{2} (g) + C l_{2} (g) ⟶ 2 H C l (g) + 184.1 k J

H C l (g) + a q ⟶ H C l (a q) + 73.2 k J

A l_{2} C l_{6} (s) + a q ⟶ A l_{2} C l_{6} (a q) + 643.1 k J

{A l}_{2} O_{3} (s)

{C r}_{2} O_{3} (s)

1596 k J

1134 k J

Δ H

{C r}_{2} O_{3} (s) + 2 A l (s) ⟶ 2 C r (s) + {A l}_{2} O_{3} (s)

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

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 .

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

Δ H

- 44

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