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Standard XII

Chemistry

Characteristics of Equilibrium Constant

In an alkalin...

Question

In an alkaline solution, the following equilibria exist.
$S^{2 -} + S \to S_{2}^{2 -}$ equilibrium constant $K_{1}$
$S_{2}^{2 -} + S \to S_{3}^{2 -}$ equilibrium constant $K_{2}$
$K_{1}$ and $K_{2}$ have the values 12 and 11, respectively.
$S_{3}^{2 -} \to S^{2 -} + 2 S$ . What is equilibrium constant for the reaction?

132

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7.58 \times 10^{- 3}

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1.09

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0.198

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Solution

The correct option is B $7.58 \times 10^{- 3}$
Given,
$S^{2 -} + S \to S_{2}^{2 -} : (K_{1}) . . . (1)$
$S_{2}^{2 -} + S \to S_{3}^{2 -} : (K_{2}) . . . (2)$

The reaction for which equilibrium constant required is,
$S_{3}^{2 -} \to S^{2 -} + 2 S$

Since the equation is obtained by reversing and adding equation (1) & (2), so the required equilibrium constant will be,
$K_{3} = \frac{1}{K_{1}} \times \frac{1}{K_{2}} = \frac{1}{12} \times \frac{1}{11} = 7.58 \times 10^{- 3}$

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Sulphide ions in alkaline solution react with solid sulphur to form polyvalent sulphide ions. The equilibrium constant for the formation of $S_{2}^{2 -}$ and $S_{3}^{2 -}$ from S and $S^{2 -}$ ions are 1.7 and 5.3 respectively. Equilibrium constant for the formation of $S_{3}^{- 2}$ from S is:

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In an alkaline solution, the following equilibria exist. S2−+S→S2−2equilibrium constant K1 S2−2+S→S2−3 equilibrium constant K2 K1 and K2 have the values 12 and 11, respectively. S2−3→S2−+2S. What is equilibrium constant for the reaction?