For which reaction will - H- E-0- Assume that each reaction is carried out in an open container-

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For which rea...

Question

For which reaction will $Δ H - Δ E = 0 ?$ Assume that each reaction is carried out in an open container.

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

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

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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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Δ H

Δ E

Δ H = Δ U

2 H_{2} O (g) ⇋ 2 H_{2} (g) + O_{2} (g); K_{1} = 6.4 \times 10^{- 8}

2 C O_{2} (g) ⇋ 2 C O (g) + O_{2} (g); K_{2} = 1.6 \times 10^{- 6}

H_{2} (g) + C O_{2} (g) ⇋ C O (g) + H_{2} O (g)

1400 K

2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g); K_{1} = 2.1 \times 10^{- 13}

2 {C O}_{2} (g) ⇌ 2 C O (g) + O_{2} (g); K_{2} = 1.4 \times 10^{- 12}

K

H_{2} (g) + C O_{2} (g) ⇌ C O (g) + H_{2} O (g)

Δ H = Δ U

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