Home
Class 11
CHEMISTRY
I(2(aq)) + I((aq))^(-) hArr I(3(aq))^(-)...

`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

A

1.33

B

2.66

C

2

D

3

Text Solution

Verified by Experts

The correct Answer is:
A
`underset(1-alpha)underset(1)(I_(2(aq)))+ underset(0.5-alpha)underset(0.5)(I_((aq))^(-)) harr underset(alpha)underset(0)(I_(3(aq))^(-))`
At equilibrium
`(0.5-alpha)` mole of `I^(-)`
reacts with `AgNO_(3)` to gave 0.25 mole of AgI
`:. 0.5 - alpha=0.25, alpha=0.25`
`K_(c)=([I_(3)^(-)])/([I_(2)](I^(-)))=(2)/((1-alpha)(0.5-alpha))=(0.25)/(0.75 xx 0.25)=(4)/(3)=1.33`
Promotional Banner

Similar Questions

Explore conceptually related problems

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.

Mole of PCl_(5) is heated in a closed vessel of 1 litre capacity. At equilibrium 0.4 moles of chlorine is found. Calculate the equilibrium constant.

3 moles of NH_3 are allowed to dissociate in a 5 litre vessel and the equilibrium concentration of N_2 is 0.2 mole/lit . Then the total number of moles at equilibrium 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

1.1 mole of A and 2.2 moles of B reach an cquilibrium in I lit container according to the reaction. A + 2B hArr 2C + D. If at equilibrium 0.1 mole of D is present, the equilibrium constant is:

Consider the following reaction equilibrium N_(2)(g)+ 3H_(2)(g) hArr 2NH_(3) Initially, 1 mole of N_(2) and 3 moles of H_(2) are taken in a 2 2L flask. At equilibrium state, if the number of moles of N_(2) is 0.6, what is the total number of moles of all gases present in the flask?

For the equilibrium in gaseous phase in 2 lit flask we start with 2 moles of SO_(2) and 1 mole of O_(2) at 3 atm, 2SO_(2(g)) + O_(2(g)) hArr 2SO_(3(g)) . When equilibrium is attained, pressure changes to 2.5 atm. Hence, equilibrium constant K_(c) is :