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Heat of Formation

Calculate the...

Question

Calculate the enthalpy of formation of anhydrous Al2Cl6 from the following data: 1. 2Al(s)+6HCl(aq)------Al2Cl6(aq)+3H2(g)=1004.2kj.kj /mol 2.H2(g) +Cl2(g)------- 2Hcl(g) =184.1kj /mol 3.HCl(g)+aq------ HCl(aq)=73.2 kj/mol 4.Al2Cl6(s) + aq-------- Al2Cl6(aq) =643.1 kj /mol

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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} 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} (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

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

H_{(a q)}^{+} + O H_{(a q)}^{-} = H_{2} O_{(l)}, Δ H = - X_{1}

m o l^{- 1}

H_{2 (g)} + \frac{1}{2} O_{2 (g)} = H_{2} O_{(l)}, Δ H = X_{2}

m o l^{- 1}

C O_{2 (g)} + H_{2 (g)} = C O_{(g)} + H_{2} O_{(l)} - X_{3}

m o l^{- 1}

C_{2} H_{2 (g)} + \frac{5}{2} O_{2 (g)} = 2 C O_{2 (g)} + H_{2} O_{(l)} + X_{4}

m o l^{- 1}

H_{2} O_{(l)}

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