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?

Question

anubhav · Answer

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 · Answer

The answer is 1.33 because at equilibrium, concentration of :- I- is .25 mol I2 is .75 mol I3- is .25 mol

Kartik · Answer

Can you please provide a more solution to this question .. please ...... Please provide the relevant equations and other necessities ...

Shruti · Answer

Keq=[I 3 ]/[I 2 ][I - ] =0.25/(0.25)(0.75) =1/0.75 =1.33 This happens because of the following reaction- I 3 +3AgNo 3 ------> 3AgI + 3No 3 when I 3 reacts with AgNo 3 it gives yellow precipitate of AgI.

Eshan Kharya · Answer

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 I 3 - gives 3 mol of AgI. So, shouldn't there be 0.25/3 mol of I 3 - to produce 0.25 mol of AgI?

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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?

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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?

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