At equilibrium which of the following reaction remains unaffected by pressure change?

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

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2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

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H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)

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2 N O_{2} (g) ⇌ N_{2} O_{4} (g)

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Solution

The correct options are
A $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$
D $H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$
The following equilibria remains unaffected by pressure change :
(A) $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$
(C) $H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$
For these equilibria, the total number of moles of gaseous reactants are equal to the total number of moles of gaseous products or $Δ n = 0$ .
The following equilibria are affected by pressure change :
(B) $2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$
(D) $2 N O_{2} (g) ⇌ N_{2} O_{4} (g)$
For these equilibria, the total number of moles of gaseous reactants are not equal to the total number of moles of gaseous products or $Δ n \neq 0$ .

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Similar questions

Δ H

Δ U

2 S O_{2 (g)} + 2 N O_{2 (g)} ⟶ 2 S O_{3 (g)} + 2 N O_{g}

2 N O_{(g)} + O_{2 (g)} ⟶ 2 N O_{2 (g)}

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

2 S O_{2 (g)} + 2 N O_{2 (g)} \to 2 S O_{3 (g)} + 2 N O_{(g)}

2 N O_{(g)} + O_{2 (g)} \to 2 N O_{2 (g)}

N_{2} (g) + O_{2} (g) \to 2 N O (g)

Δ H = 181

2 C O_{2} (g) \to 2 C O (g) + O_{2} (g); Δ H = 566

H_{2} (g) + I_{2} (g) \to 2 H I (g); Δ H = - 94

H_{2} (g) + F_{2} (g) \to 2 H F (g); Δ H = - 541

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