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Le Chatelier's Principle

Which of the ...

Question

Which of the following reactions proceed in forward direction with an increase in temperature?

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g) + 3000 c a l

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N_{2} (g) + O_{2} (g) ⇌ 2 N O (g) - 43200 c a l

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N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g) + 22400 c a l

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C (g) + O_{2} (g) ⇌ C O_{2} (g) + 94300 c a l

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Solution

The correct option is B $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g) - 43200 c a l$
Option (B) is correct.
Endothermic reactions are favoured with the increase in temperature. In an endothermic reaction, an increase in temperature favours the reaction to occur in the forward direction. It means heat is absorbed by the reactants. When the temperature of an equilibrium mixture is increased, the rate of both reactions increases but the rate of the endothermic reaction (the reaction that absorbs the added energy) is increased more.

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Similar questions

2 H I_{(g)} ⟶ H_{2 (g)} + I_{2 (g)}

2 N H_{3 (g)} ⟶ N_{2 (g)} + 3 H_{2 (g)}

2 N O_{(g)} ⟶ N_{2 (g)} + O_{2 (g)}

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

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

Δ H = + 172.5

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

Δ H = - 91.8

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

Δ H = + 181

2 H_{2} O (g) \to 2 H_{2} (g) + O_{2} (g); Δ H = 484.6

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

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); K_{2}

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}

2 N H_{2} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)

\frac{K_{p}}{K_{c}}

300 K

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

[A t 300 K, R T = 24.62 d m^{3} a t m m o l^{- 1}]

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