For which reaction will - H - - U- Assume each reaction is carried out in an open container-

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For which rea...

Question

For which reaction will $Δ H = Δ U$ ?

Assume each reaction is carried out in an open container.

H_{2} (g) + B r_{2} (g) ⟶ 2 H B r (g)

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C (s) + 2 H_{2} O (g) ⟶ 2 H_{2} (g) + C O_{2} (g)

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4 C O (g) + 2 O_{2} (g) ⟶ 4 C O_{2} (g)

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2 P C l_{5} (g) ⟶ 2 P C l_{3} (g) + 2 C l_{2} (g)

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Δ H = Δ U

Δ H

Δ E

Δ H - Δ E = 0 ?

Determine $Δ U^{\circ}$ at 300 K for the following reaction using the listed enthalpies of reaction.

$4 C O (g) + 8 H_{2} (g) \to 3 C H_{4} (g) + C O_{2} (g) + 2 H_{2} O (l)$

$C (g r a p h i t e) + \frac{1}{2} O_{2} (g) \to C O (g); Δ {H_{1}}^{\circ} = - 110.5 k J$

$C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g); Δ {H_{2}}^{\circ} = - 282.9 k J$

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H_{3}^{0} = - 285.8 k J$

$C (g r a p h i t e) + 2 H_{2} (g) \to C H_{4} (g); Δ H_{4}^{0} = - 74.8 k J$

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (g)

Δ H

Δ U

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