**Problem Statement:**A quantity of HI was sealed in a tube, heated to 425°C, and held at this temperature until equilibrium was reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 mol/L. Calculate the equilibrium concentration of H₂ (and I₂). For the gas-phase reaction:\[ \text{H}_2 + \text{I}_2 \leftrightarrow 2\text{HI} \]The equilibrium constant \( K_c \) at 425°C is 54.6.**Options:**(a) \( 9.55 \times 10^{-3} \, \text{M} \)(b) \( 1.17 \times 10^{-3} \, \text{M} \)(c) \( 1.85 \times 10^{-4} \, \text{M} \)(d) \( 4.78 \times 10^{-3} \, \text{M} \)(e) \( 2.34 \times 10^{-3} \, \text{M} \)

Step 1) equilibrium constant is defined as the ratio of the equilibrium concentrations of products…

9. A quantity of HI was sealed in a tube, heated to 425°C and held at this temperature until equilibrium was reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 mol/L. Calculate the equilibirum concentration of H2 (and I2). For the gas-phase reaction, H2 + 12 2HI Kc = 54.6 at 4250C %3D

9. A quantity of HI was sealed in a tube, heated to 425°C and held at this temperature until equilibrium was reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 mol/L. Calculate the equilibirum concentration of H2 (and I2). For the gas-phase reaction, H2 + 12 2HI Kc = 54.6 at 4250C %3D

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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