`I_(2)+I^(ɵ)hArrI_(3)^(ɵ)`
This reaction is set-up in aqueous medium. We start with `1` mol of `I_(2)` and `0.5` mol of `I^(ɵ)` in `1 L` flask. After equilibrium reached, excess of `AgNO_(3)` gave `0.25` mol of yellow precipitate. Equilibrium constant is

I_(2(aq)) + I_((aq))^(-) hArr I_(3(aq))^(-). We started with I mole of I_(2) and 0.5 mole of l^(-) in one litre flask. After equilibrium is reached, excess of AgNO_(2) gave 0.25 mole of yellow precipitate. Equilibrium constant is

0.5 mol of H_(2) and 0.5 mole of I_(2) react in 10 litre flask at 448^(@)C . The equilibrium brium constant K_(C) is 50 for H_(2)(g)I_(2)(g) hArr 2HI(g) Calcualte mole of I_(2) at equilibrium.

1.1 mol of A is mixed with 2.2 mol of B and the mixture is kept in a one - itre flask till the equilibrium, A+2BhArr 2C+D is reached. At equilibrium 0.2 mol of C is formed. The equilibrium constant of the above reaction is

In this process I_(2) + I^(-) hArr I_(3)^(-) (in aq medium) , initially there are 2 mole I_(2) & 2 mole I^(-) . But at equilibrium due to addition of AgNO_(3 (aq)) , 1.75 mole yellow ppt is obtained . K_(C) for the process is ( V_("flask") = 1 dm^(3) ) nearly