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Characteristics of Equilibrium Constant

I2+I-⇌ I3-Thi...

Question

$I_{2} + I^{-} ⇌ I_{3}^{-}$ This reaction is set-up in aqueous medium. We start with one mole of $I_{2}$ and $0.5 m o l$ of $I^{-}$ in $1 L$ flask. After equilibrium is reached, excess of $A g N O_{3}$ gave $0.25 m o l$ of yellow precipitate. Equilibrium constant is

A

1.33

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B

2.66

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C

2.00

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D

3.00

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Solution

The correct option is A $1.33$

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Similar questions

I_{2} + I^{-} ⇌ I_{3}^{-}

. This reaction is set up in aqueous medium. We start with

1

I_{2}

0.5

I^{-}

1

L flask. After equilibrium, the excess of

A g N O_{3}

0.25

moles of yellow ppt. Then the equilibrium constant is:

I_{2} (a q) + I^{-} (a q) ⇌ I_{3}^{-} (a q) .

We started with 1 mole of

I_{2}

and 0.5 mole of

I^{-}

in one litre flask. After equilibrium is reached, excess of

A g N O_{3}

gave 0.25 mole of yellow precipitate. Equilibrium constant is:

I_{2} (a q) + I^{-} (a q) ⇌ I_{3}^{-} (a q) .

We started with

1

I_{2}

0.5

I^{-}

in one litre flask. After equilibrium is reached excess of

A g N O_{3}

0.25

mole of yellow precipitate. Equilibrium constant is:

Q. For the reaction :

X_{2} + X^{-} ⇌ X_{3}^{-} (X = i o d i n e)

. This reaction is set up in aqueous medium. We start with 1 mol of

X_{2}

X^{-}

in 1L flask. After equilibrium is reached, excess of

A g N O_{3}

gave 0.25 mol of yellow ppt. Equilibrium constant is :

I- ion react with iodine in aqueous solution to form I3- ion .When 1L of solution containing 1mole of KI and 0.25 mol of I2 was reacted with excess of AgNO3 ,0.80 mol of yellow precipitate was formed.The stability constant of. I3- ion is

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