1 mole each of $N_{2} (g)$ and $O_{2} (g)$ are introduced in a $1 L$ evacuated vessel at $523 K$ and equilibrium $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ is establised. The concentration of $N O (g)$ at equilibrium.

Changes on changing volume of the vessel

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Changes on changing temperature

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Changes on changing pressure

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Remains same even when a platinum gauze is introduced to catalyse the reaction.

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Solution

The correct options are
A Changes on changing volume of the vessel
B Changes on changing temperature
C Changes on changing pressure
D Remains same even when a platinum gauze is introduced to catalyse the reaction.
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$

(A) Volume change will change concentration, not the number of moles.

(B) Temperature change will change $K_{p}$ and hence concentration.

(C) For changing pressure, volume has to be changed, though number of moles of $N O (g)$ do not get, changed but its concentration will get changed.

(D) Catalyst does not change equilibrium concentrations.

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Similar questions

Q. Assertion :A change of pressure has no effect in case of the equilibrium,

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

Reason: The reaction,

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

is highly exothermic reaction.

The equilibrium constant at 850 K for the reaction
$N_{2} (g) + O_{2} (g) ⇋ 2 N O (g)$ is 0.5625. The equilibrium concentration of $N O (g)$ is $3.0 \times 10^{-} 3 M$
If the concentration of $N_{2} (g)$ and $O_{2} (g)$ are equal, the concentration of $N_{2} (g)$ in M is: