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Characteristics of Equilibrium Constant

In the reacti...

Question

In the reaction, $H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$ , in a $2$ litre flask $0.4$ mole of each $H_{2}$ and $I_{2}$ are taken. At equilibrium $0.5$ mol of $H I$ are formed. What will be the value of equilibrium constant $K_{c}$ ?

20.2

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25.4

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0.284

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11.1

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Solution

The correct option is D $11.1$
In the reaction, $H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$ , in a $2$ litre flask $0.4$ mole of each $H_{2}$ and $I_{2}$ are taken. At equilibrium $0.5$ mol of $H I$ are formed. The value of equilibrium constant $K_{c}$ will be $11.1$ .
0.5 moles of HI will be obtained from 0.25 moles of $H_{2}$ and 0.25 moles of $I_{2}$ .
$0.4 - 0.25 = 0.15$ moles of $H_{2}$ and $0.4 - 0.25 = 0.15$ moles of $I_{2}$ will remain.
The equilibrium constant

$K_{c} = \frac{[H I]^{2}}{[H_{2}] [I_{2}]}$

$K_{c} = \frac{(\frac{0.5 mol}{2 L})^{2}}{(\frac{0.15 mol}{2 L}) \times (\frac{0.15 mol}{2 L})}$

$K_{c} = 11.1$

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In the reaction, H2(g)+I2(g)⇌2HI(g), in a 2 litre flask 0.4 mole of each H2 and I2 are taken. At equilibrium 0.5 mol of HI are formed. What will be the value of equilibrium constant Kc?

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