Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI (g) ⇌H2 (g) + I2 (g) At equilibrium it is found that [HI] = 3.5210-3 M, [H2] = 4.7810-4 M, and [I2] = 4.78*10-4 M. You may want to reference (pages 644 - 645) Section 15.5 while completing this problem. Part A What is the value of Kc at this temperature? Express the equilibrium constant to three significant digits

Question

Chemistry

Magdalena Moses

10 May, 09:07

Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI (g) ⇌H2 (g) + I2 (g) At equilibrium it is found that [HI] = 3.5210-3 M, [H2] = 4.7810-4 M, and [I2] = 4.78*10-4 M. You may want to reference (pages 644 - 645) Section 15.5 while completing this problem. Part A What is the value of Kc at this temperature? Express the equilibrium constant to three significant digits

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Answers (1)

Know the Answer?

Lea Hicks · Answer 1

0.0184

Explanation:

Let's consider the following reaction at equilibrium.

2 HI (g) ⇌ H₂ (g) + I₂ (g)

The concentration equilibrium constant (Kc) is equal to the product of the concentration of the products raised to their stoichiometric coefficients divided by the product of the concentration of the reactants raised to their stoichiometric coefficients.

Kc = [H₂] * [I₂] / [HI]²

Kc = (4.78 * 10⁻⁴) * (4.78 * 10⁻⁴) / (3.52 * 10⁻³) ²

Kc = 0.0184