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Characteristics of Equilibrium Constant

The following...

Question

The following water gas shift reaction is an i portant industrial process for the prodicution of hydrogen gas.
$C O (g) + H_{2} O (g) ⇌ C O_{2} (g) + H_{2} (g)$
At a given temperature $K_{p} = 2.7$ . If $0.13 m o l$ of $C O, 0.56 m o l$ of water, $0.78 m o l$ of $C O_{2}$ and $0.28 m o l$ of $H_{2}$ are introduced into a $2 L$ flask, and find out in which direction must the reaction proceed to reach equilibrium:

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Solution

At a given temp $K_{e q} = 2.7$

At given time, $Q = \frac{[C O_{2}] [H_{2}]}{[C O] [H_{2} O]} = \frac{0.78 \times 0.28}{0.13 \times 0.56}$

$Q = 3$

Since $Q > K_{e q}$ (as $3 > 2.7$ )

The concentration of products is more so reaction occurs in backward direction

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