Consider 1.70 mol of carbon monoxide and 3.00 mol of chlorine sealed in a 3.00 L container at 476 °C. The equilibrium constant, Ke, is 2.50 (in M-¹) for CO(g) + Cl₂(g) → COCl2(g) Calculate the equilibrium molar concentration of CO. Answer: 0.144

Consider 1.70 mol of carbon monoxide and 3.00 mol of chlorine sealed in a 3.00 L container at 476 °C. The equilibrium constant, Ke, is 2.50 (in M-¹) for CO(g) + Cl₂(g) → COCl2(g) Calculate the equilibrium molar concentration of CO. Answer: 0.144

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 118CP: Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain...

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Question

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Consider 1.70 mol of carbon monoxide and 3.00 mol of chlorine sealed in a 3.00 L
container at 476 °C. The equilibrium constant, Kc, is 2.50 (in M-¹) for
CO(g) + Cl₂(g) → COCl2(g)
Calculate the equilibrium molar concentration of CO.
Answer: 0.144
For the reaction:
2HI (g) → H₂ (g) + 12 (g)
Keq = 0.016
Initially a container contains 0.37 M of HI and no product. What is the equilibrium
concentration of H₂?
Answer: 0.0415

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