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The elementary reaction 2 H 2 O ( g ) − ⇀ ↽ − 2 H 2 ( g ) + O 2 ( g ) proceeds at a certain temperature until the partial pressures of H 2 O , H 2 , and O 2 reach 0.0150 bar , 0.00550 bar , and 0.00500 bar respectively. What is the value of the equilibrium constant at this temperature?

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dsdrajlin

Answer:

6.72 × 10⁻⁴

Explanation:

Let's consider the following elementary reaction.

2 H₂O(g) ⇄ 2 H₂(g) + O₂(g)

The equilibrium constant (Kp) is the product of the partial pressures of the products raised to their stoichiometric coefficients divided by the product of the partial pressures of the reactants raised to their stoichiometric coefficients.

[tex]Kp=\frac{pH_{2}^{2}.pO_{2} }{pH_{2}O^{2} } =\frac{(0.00550)^{2}.(0.00500)}{(0.0150)^{2} } =6.72 \times 10^{-4}[/tex]

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