For which reaction will - H- U -

The correct option is A H_2(g)+Br_2(g)→ 2HBr(g) Δ H = Δ U + PΔ V Δ H = Δ U + Δ n_gRT In only reaction (A) the #160; Δ n_g = 0 and hence ...

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Calorimetry

For which rea...

Question

For which reaction will $Δ H = Δ U$ ?

H_{2} (g) + B r_{2} (g) \to 2 H B r (g)

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

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

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2 C O (g) + O_{2} (g) \to 2 C O_{2} (g)

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Δ H > Δ U

Δ H < Δ U

C (g r a p h i t e) + O_{2} (g) ⟶ C O_{2} (g)

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

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

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)

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94 k c a l

2 C O (g) + O_{2} (g) \to 2 C O_{2} (g); Δ H = - 135.2 k c a l

C 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)

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