Question

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 0.0500 atm, 0.00150 atm, and 0.00150 atm, respectively. What is the value of the equilibrium constant at this temperature?

Answer 1

6.75 × 10⁻⁸is the value of the equilibrium constant at this temperature.

Step-by-step explanation:

2H₂O(g) ⇄ 2H₂(g) + O₂(g)

Partial pressure of H₂O = 0.0500 atm

Partial pressure of H₂ = 0.00150 atm

Partial pressure of O₂ = 0.00150 atm

The expression of Kp for the given chemical equation is:

`K_p = ([H_2]^2[O_2])/(H_2O)`

`= ((0.00150^2)(0.00150))/((0.0500)) \\= 6.75 * 10^-^8`

6.75 × 10⁻⁸is the value of the equilibrium constant at this temperature