Chemistry: 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 0.025 atm, 0.0060 atm, and 0.0090 atm, respectively at equilibrium. What is the value of the equilibrium constant at this temperature?

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The elementary reaction 2 H 2 O ( g ) − ⇀ ↽ − 2

emzaa

21.01.2022

The value of equilibrium constant = 0.005184

Explanation:

According to the given reaction we consider Kp equation and find the value of equilibrium constant using partial pressure of individual gases.

2 H 2 O ( g ) ⇄ 2 H 2 ( g ) + O 2 ( g )

Kp = $\frac{Partial pressure of products}{Partial pressure of reactants}$

$K_{p} = \frac{P_{H_{2}^{2} }X P{o_{2} } }{P_{H_{2}O^{2} } }$

Change of gaseous moles(Δn)

= 3 - 2

= 1

⇒ $K_{p} = \frac{(0.006)^{2}X(0.009) }{(0.025)^{2} } \\Kp = 0.005184$

∴ The value of equilibrium constant = 0.005184

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