The elementary reaction 2 H 2 O ( g ) − ⇀ ↽ − 2 H 2 ( g ) + O 2 ( g ) 2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H 2 O , H2O, H 2 , H2, and O 2 O2 reach 0.0500 atm, 0.0500 atm, 0.00150 atm, 0.00150 atm, and 0.00150 atm, 0.00150 atm, respectively. What is the value of the equilibrium constant at this temperature?

K = 0,00000135 = 1.35 * 10^-6

Explanation:

Step 1: Data given

The equilibrium constant, K, for any reaction is defined as the concentrations of the products raised by their coefficients divided by the concentrations of the reactants raised by their coefficients. In this case, the concentrations are given as partial pressures.

The partial pressures of H2O = 0.0500 atm

The partial pressures of H2 = 0.00150 atm

The partial pressures of O2 = 0.00150 atm

Step 2: The balanced equation

2H2O(g) ⇆ 2H2(g) + O2(g)

Step 3: Calculate K

K = [O2][H2]² / [H2O]²

K = 0.00150 * 0.00150² /  0.0500²

K = 0,00000135 = 1.35 * 10^-6

the temperature of the gas, in k, not celsius.

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