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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 0.015 bar, 0.0080 bar, and 0.0080 bar, respectively. What is the value of the equilibrium constant at this temperature?

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jufsanabriasa

Answer:

Kp = 2.28x10⁻³

Explanation:

For the reaction:

2H₂O(g) ⇄ 2H₂(g) + O₂(g)

The equilibrium constant written in terms of partial pressures, Kp, is defined as:

[tex]Kp = \frac{P[H_2]^2P[O_2]}{P[H_2O]^2}[/tex](1)

Replacing the partial pressure of each compound in the formula:

[tex]Kp = \frac{0.0080bar^20.0080bar}{0.015bar^2}[/tex]

Kp = 2.28x10⁻³

That means the equilibrium constant is 2.28x10⁻³

I hope it helps!

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