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i2 + i- i3- this reaction is setup in an aqueous medium. we start with 1mol of i2 and 0.5mol of i- in 1litre flask. after equilibrium is reached, excess of agno3 gave 0.25 mol of yellow precipitate. whats the equilibrium constant?

i2 + i- i3- this reaction is setup in an aqueous medium. we start with 1mol of i2 and 0.5mol of i- in 1litre flask. after equilibrium is reached, excess of agno3 gave 0.25 mol of yellow precipitate. whats the equilibrium constant?

Grade:11

5 Answers

anubhav
34 Points
5 years ago
4/3. This is because conc. Of i- ion at equilibrium is 0.25mol and that of i2 is 0.75 and of i3- is 0.25
Sahil Saha
12 Points
4 years ago
The answer is 1.33 because at equilibrium, concentration of :-
I- is .25 mol
I2 is .75 mol
I3- is .25 mol
Kartik
16 Points
4 years ago
Can you please provide a more solution to this question .. please ...... Please provide the relevant equations and other necessities ...
Shruti
11 Points
4 years ago
Keq=[I 3]/[I 2][I -]
        =0.25/(0.25)(0.75)
        =1/0.75
        =1.33
This happens because of the following reaction-
3 +3AgNo------>3AgI + 3No3 when I  reacts with AgNo 3  it gives yellow precipitate of AgI.
Eshan Kharya
19 Points
2 years ago
Hi. Silly doubt. It says 0.25 mol of yellow ppt is formed. The yellow ppt is AgI. However, according to the reaction, 1 mol of I3- gives 3 mol of AgI. So, shouldn't there be 0.25/3 mol of I3to produce 0.25 mol of AgI?
 

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