For the reaction : $2 N O_{(g)} ⇌ N_{2 (g)} + O_{2 (g)}$ ; $Δ H = -$ heat
$K_{e} = 2.5 \times 10^{2}$ at $298 K$
What will happen to the concentration of $N_{2}$ if :
(1) Temperature is decreased to $273 K$ .
(2) Pressure is reduced.

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Solution

(1) If temperature is decreased to $273 K$ , then the concentration of $N_{2}$ will decreases, according to LeChatelier principle, the reaction is favoured to backward direction.
(2) There is no change in the concentration of $N_{2}$ when pressure is reduced since for the reversible reaction which proceed with no change in volume, pressure has no effect on the position of equilibrium.

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