Ask Question
16 October, 15:25

Gaseous hydrogen iodide is placed in a closed container at 425 degrees C, where it partially decomposes to hydrogen and iodine: 2HI (g) - -->/<---H2 (g) + I2 (g). At equilibrium it is found that [HI] = 3.59

+2
Answers (1)
  1. 16 October, 15:28
    0
    0.0184

    Explanation:

    There is some info missing. I think this is the original question.

    Gaseous hydrogen iodide is placed in a closed container at 425 °C, where it partially decomposes to hydrogen and iodine: 2 HI (g) ⇄ H₂ (g) + I₂ (g). At equilibrium, it is found that HI = 3.59 * 10⁻³ M, H₂ = 4.87 * 10⁻⁴ M, and I₂ = 4.87 * 10⁻⁴ M.

    What is the value of Kc at this temperature?

    Express the equilibrium constant to three significant digits.

    Let's consider the following reaction at equilibrium.

    2 HI (g) ⇄ H₂ (g) + I₂ (g)

    The concentration equilibrium constant (Kc) is 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 = 4.87 * 10⁻⁴ * 4.87 * 10⁻⁴ / (3.59 * 10⁻³) ²

    Kc = 0.0184
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Gaseous hydrogen iodide is placed in a closed container at 425 degrees C, where it partially decomposes to hydrogen and iodine: 2HI (g) - ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers