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 $$\mathrm{N}{\phantom{A}}_2\mathrm{O}{\phantom{A}}_4\stackrel{-\rightharpoonup }{\leftharpoondown -}2\mathrm{NO}{\phantom{A}}_2$$ is ______.

पर्याय

• 0.01 × 10⁻³

• 2 × 10⁻³

• 2 × 10⁻⁵

• 1 × 10⁻⁵

Answer 1

1 × 10⁻⁵

Explanation:

	$$\mathrm{N}{\phantom{A}}_2\mathrm{O}{\phantom{A}}_4$$	$$\stackrel{-\rightharpoonup }{\leftharpoondown -}$$	$$2\mathrm{NO}{\phantom{A}}_2$$
At equilibrium	${\displaystyle \frac{0.2}{2}}$		${\displaystyle \frac{2\times {10}^{-3}}{2}}$
	0.1		1 × 10–3

K_c = ${\displaystyle \frac{{\left[{\text{NO}}_2\right]}^2}{\left[{\text{N}}_2{\text{O}}_4\right]}}$

= ${\displaystyle \frac{{(1\times {10}^{-3})}^2}{0.1}}$

= 1 × 10⁻⁵