9.2 grams of N_(2)O_(4) (g) is taken in a closed one litre vessel and heated till the following equilibrium is reachedN_(2) O_(4) (g) hArr 2 NO_(2) (g) At equilibrium , 50% N_(2)O_(4) (g) is dissociated . What is the equilibrium constant ( in mol lit^(-1)) (" Molecular weughtof" N_(2)O_(4) = 92)

9.2 grams of N_(2)O_(4) (g) is taken in a closed one litre vessel and

1.	9.2 grams of N_(2)O_(4) (g) is taken in a closed one litre vessel and heated till the following equilibrium is reachedN_(2) O_(4) (g) hArr 2 NO_(2) (g) At equilibrium , 50% N_(2)O_(4) (g) is dissociated . What is the equilibrium constant ( in mol lit^(-1)) (" Molecular weughtof" N_(2)O_(4) = 92)
Answer» `0.1` `0.2` `0.4` 2 Solution :Intial` [N_(2)O_(4)] = 9.2//92 " mol"L^(-1) = 0.1 " mol "L^(-1)` At. Eqm. ( after 50% dissociation ), `[N_(2)O_(4)] = 0.05 M, [NO_(2)] = 0.1 M` ` K = ([NO_(2)])/([N_(2)O_(4)])=(0.1)^(2)/0.05 = 0.2`