Hydrogen iodide decomposes according to the equation:\[ 2 \text{HI(g)} \rightleftharpoons \text{H}_2\text{(g)} + \text{I}_2\text{(g)} \]For which \( K_c = 0.0156 \) at 400°C. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400°C. What is the concentration of \(\text{H}_2\) at equilibrium?

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Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + 12(g), for which Kc = 0.0156 at 400°C. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400°C. What is the concentration of H₂ at equilibrium?

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + 12(g), for which Kc = 0.0156 at 400°C. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400°C. What is the concentration of H₂ at equilibrium?

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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