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9.2 grams of N(2)O(4(g)) is taken in a c...

`9.2` grams of `N_(2)O_(4(g))` is taken in a closed one litre vessel and heated till the following equilibrium is reached `N_(2)O_(4(g))hArr2NO_(2(g))`. At equilibrium, `50% N_(2)O_(4(g))` is dissociated. What is the equilibrium constant (in mol `litre^(-1)`) (Molecular weight of `N_(2)O_(4) = 92`) ?

A

`0.1`

B

`0.2`

C

`0.4`

D

2

Text Solution

Verified by Experts

The correct Answer is:
B
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`
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