Which of the following will shift the equilibrium in the forward direction for the following equilibrium?
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ ; $Δ H^{0} = + 181 k J$ .

Increase of pressure

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Increase in the concentration of

N O

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Decrease in pressure

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Increase in temperature

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Solution

The correct option is D Increase in temperature
The equilibrium reaction is $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ . The positive value of $Δ H$ indicates that the reaction is endothermic in nature.

When the temperature is increased, the equilibrium will shift in the forward direction so that the heat is absorbed, which will nullify the effect of the increase in temperature.

Suggest Corrections

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N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g) + h e a t

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

N_{2} (g) + O_{2} (g) ⇋ 2 N O (g)

C a C O_{3} (s) \to C a O (s) + C O_{2} (g)

Δ_{f} H^{o} [C a O (s)] = - 635.1 {kJ mol}^{- 1}

Δ_{f} H^{o} [C O_{2} (g)] = - 393.5 {kJ mol}^{- 1}

Δ_{f} H^{o} [C a C O_{3} (s)] = - 1206.9 {kJ mol}^{- 1}

N_{2} (g)

O_{2} (g)

1 L

523 K

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

N O (g)

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