Chemical EquilibriumHard

Question

Iron fillings and water were placed in a 5 L vessel and sealed. The tank was heated to 1000oC. Upon analysis, the tank was found to contain 1.2 g of H2(g) and 54.0 g of H2O(g). If the reaction is represented as

3Fe(s) + 4H2O(g) $\rightleftharpoons$Fe3O4(s) + 4H2(g), then the value of equilibrium constant is

Options

A.0.2
B.0.04
C.0.008
D.0.0016

Solution

CO2(g) + C(s) $\rightleftharpoons$ 2CO(g)

Given: a mole 9a mole

Required: b mole 4b mole

Now, $K_{p} = \frac{\left( \frac{9a}{10a} \times 16 \right)^{2}}{\left( \frac{a}{10a} \times 16 \right)} = \frac{\left( \frac{4b}{5b} \times P \right)^{2}}{\left( \frac{b}{5b} \times P \right)}$

⇒ P = 40.5 atm

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