Question

The decomposition of N₂O₄ to NO₂ was carried out in chloroform at 280°C. At equilibrium, 0.2 mol of N₂O₄ and 2 × 10⁻³ mol of NO₂ were present in 2 ℓ of the solution. The equilibrium constant for the reaction \[\ce{N2O4 <=> 2NO2}\] is ______.

पर्याय

• 0.01 × 10⁻³

• 2 × 10⁻³

• 2 × 10⁻⁵

• 1 × 10⁻⁵

Answer 1

1 × 10⁻⁵

Explanation:

	\[\ce{N2O4}\]	\[\ce{<=>}\]	\[\ce{2NO2}\]
At equilibrium	`0.2/2`		`(2 xx 10^-3)/2`
	0.1		1 × 10–3

K_c = `(["NO"_2]^2)/(["N"_2"O"_4])`

= `(1 xx 10^-3)^2/0.1`

= 1 × 10⁻⁵