Nitrogen dioxide froms dinitrogen tetroxide according to the equation
`2NO_(2)(g)hArrN_(2)O_(4)` (g) when 0.1 mole of `NO_(2)` is added to a 1 litre flask at `25^(@)C`, the concentration changes so that at equilibrium `[NO_(2)]=0.016M` and `[N_(2)O_(4)]=0.042M`.
a. What is the value of the reaction Quotient before any reaction occurs.
b. What is the value of the equilibrium constant for the reaction.

Explanation

a. `2NO_(2)hArrN_(2)O_(4)`
Reaction quotient `Q=([N_(2)O_(4)])/([NO_(2)]^(2))=0/0.1=0`
b. `underset(0.016)(2NO_(2))hArr underset(0.042)(N_(2)O_(4))`
`K_(c)=([N_(2)O_(4)])/([NO_(2)]^(2))=0.042/([0.016]^(2))=1.64xx10^(2)`