Calculate the Equilibrium Concentrations of Gases in a Reaction

What are the equilibrium concentrations of each gas at 430 °C in the reaction H₂(g) + I₂(g) ↔ 2HI(g)?

Given initial concentrations of H₂, I₂, and HI, how can we calculate the equilibrium concentrations of each gas at 430 °C?

Equilibrium Concentrations Calculation

The equilibrium concentrations of the gases at 430 °C in the reaction H₂(g) + I₂(g) ↔ 2HI(g) are [H₂] = 0 M, [I₂] = 0 M, and [HI] = 0.724 M.

To calculate the equilibrium concentrations of each gas at 430 °C in the reaction H₂(g) + I₂(g) ↔ 2HI(g), we need to use the equilibrium constant (Kc) and the initial concentrations of the gases.

Given that Kc = 54.3, and the initial concentrations are [H₂] = 0.482 M, [I₂] = 0.314 M, and [HI] = 0.879 M, we can set up an ICE table to calculate the equilibrium concentrations.

Using the equation for Kc, we can write: Kc = [HI]² / ([H₂] [I₂]).

Plugging in the given values, we have: 54.3 = [HI]² / (0.482 * 0.314).

Solving for [HI], we find that [HI] = 0.724 M.

Using the balanced reaction equation, we find [H₂] = 0 M and [I₂] = 0 M at equilibrium.

Therefore, the equilibrium concentrations of the gases are: [H₂] = 0 M, [I₂] = 0 M, and [HI] = 0.724 M.

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