What is the Value of Equilibrium Constant for a Given Reaction at 853 K?

The Equilibrium Constant for a Chemical Reaction

The value of the equilibrium constant (Kc) at 853 K for the given reaction is approximately 8.81e-5. The quantitative representation of a chemical reaction's state at equilibrium is the equilibrium constant, abbreviated as K. It is described as the ratio of the reactant and product concentrations (or partial pressures for gas-phase reactions), each concentration being raised to the power of the corresponding stoichiometric coefficient in the balanced chemical equation.

The equilibrium constant, denoted as Kc, is a measure of the extent of a chemical reaction at equilibrium. For the given reaction:

2 HI(g) ⇌ H2(g) + I2(g)

The equilibrium constant expression is:

Kc = [H2][I2] / [HI]^2

Where [H2], [I2], and [HI] are the molar concentrations of H₂, I₂, and HI, respectively, at equilibrium.

Given data:

[HI] = 0.182 M

[H2] = 2.53e-2 M

[I2] = 3.28e-2 M

Plugging these values into the equilibrium constant expression, we get:

Kc = (2.53e-2) * (3.28e-2) / (0.182)^2

Kc = 8.81e-5

What is the value of the equilibrium constant for the given reaction at 853 K?

The value of the equilibrium constant (Kc) at 853 K for the given reaction is approximately 8.81e-5.

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