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9.2g of N₂O_4(g) is taken in 1lit vessel and heated. At equilibrium, 50% is dissociated. Equilibrium constant in (mol/lit) for the reaction N₂O_4(g) $⇌$ 2NO_2(g) is

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0.1

0.2

0.4

answer is B.

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Detailed Solution

Initial moles of N₂O₄

Number of moles of N₂O₄ decomposed = 0.1 x 0.5 = 0.05

1 mole of N₂O₄(g) → 2 moles of NO₂

0.05 mole of N₂O₄(g) → 'x' moles of NO₂

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	$large 2{N_2}{O_4}left( g right)$	$large rightleftharpoons$	$large 2N{O_2}left( g right)$
Initial moles	0.1
Moles at eqbm	(0.1 - 0.05)		0.1
Eqbm. conc.	$large frac{{0.05}}{1}$		$large frac{{0.1}}{1}$	$large left ( because Volume;of;the;vessel=1lit right )$