Answer:
The answer is D - Keq = [H2]^2 × [O2]
[2]^2
Step-by-step explanation:
The equilibrium constant (Keq), is a quantitative measure of the position of equilibrium in a chemical reaction. It is defined by the ratio of the concentrations (or partial pressures) of the products to the concentrations (or partial pressures) of the reactants.
For a general chemical reaction:
aA+bB + CC+dD
Explanation: The equilibrium constant expression is given by:
Keq = [C]^c x [D]^d
[A]^a x [B]^b
Where [A], [B], [C], and [D] represent the molar concentrations of the species A, B, C, and D, respectively. The coefficients a, b, c, and d represent the stoichiometric coefficients of the balanced equation.
The given reaction is 2H2O(g) ↔ 2H2(g) + O2(g)
The equilibrium constant expression for the given system can be expressed as follows:
Keq = [H2]^2 × [O2]
[2]^2
Where:
[H2] represents the molar concentration of hydrogen gas (H2).
[O2] represents the molar concentration of oxygen gas (O2).
[H2O] represents the molar concentration of water vapor (H2O).
The equilibrium constant expression for the given system can be expressed as follows: Keq = [H2]^2 × [O2]
[2]^2