I’m stuck. I keep getting it wrong. **Equilibrium Constant Calculation: Decomposition of Hydrogen Iodide**In this exercise, gaseous hydrogen iodide (HI) is placed in a closed container at 425°C, where it partially decomposes into hydrogen (H₂) and iodine (I₂). The chemical equilibrium reaction is represented as:\[ 2\text{HI}(g) \rightleftharpoons \text{H}_2(g) + \text{I}_2(g) \]At equilibrium, the following concentrations are observed:- $[\text{HI}] = 3.59 \times 10^{-3}\, M$- $[\text{H}_2] = 4.87 \times 10^{-4}\, M$- $[\text{I}_2] = 4.87 \times 10^{-4}\, M$**Part A:****Question:** What is the value of $ K_c $ at this temperature?**Instruction:** Express the equilibrium constant ($ K_c $) to three significant digits.**Input Box:**\[ K_c = \]**Submitted Answer:**\[ 54.3 \]**Feedback:**- **Incorrect; Try Again. 5 attempts remaining.**- **Explanation:** The equilibrium constant, $ K_c $, of a reaction is the ratio of the molar concentrations of the products over the reactants, raised to the power of their stoichiometric coefficients. The answer provided corresponds to the ratio of the reactants over the products, which is incorrect.**Next Steps:** Review your calculations and attempt submission again.**Additional Resources:**- [Constants]- [Periodic Table]For more detailed guidance, refer to the related instructional materials on calculating equilibrium constants.

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] = 3.59×10-3 M . [H₂] = 4.87×104 M, and [I2] = 4.87x10-4 M. ▼ Part A What is the value of Ke at this temperature? Express the equilibrium constant to three significant digits. K₁= 54.3 Submit 195| ΑΣΦ Provide Feedback Previous Answers Request Answer Review | Constants I Periodic 1 ? X Incorrect; Try Again; 5 attempts remaining The equilibrium constant, Ke, of a reaction is the ratio of the molar concentrations of the products over the reactants. The answer you provided corresponds to the ratio of the reactants over the products. Next

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] = 3.59×10-3 M . [H₂] = 4.87×104 M, and [I2] = 4.87x10-4 M. ▼ Part A What is the value of Ke at this temperature? Express the equilibrium constant to three significant digits. K₁= 54.3 Submit 195| ΑΣΦ Provide Feedback Previous Answers Request Answer Review | Constants I Periodic 1 ? X Incorrect; Try Again; 5 attempts remaining The equilibrium constant, Ke, of a reaction is the ratio of the molar concentrations of the products over the reactants. The answer you provided corresponds to the ratio of the reactants over the products. Next

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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