8. A sealed vessel contains 0.25 M COC12, 0.11 M CO, and 0.11 M Cl2 at 668 K, which is an equilibrium mixture at this temperature. COCl2(g) = CO(g) + Cl2(g) a. When the temperature is increased and equilibrium is re-established, [COC12] = 0.18 M. Is the reaction endothermic or exothermic? How do you know? b. To the equilibrium mixture at 668 K, 0.25 M CO is added. Calculate the concentration of each gas at equilibrium.

8. A sealed vessel contains 0.25 M COC12, 0.11 M CO, and 0.11 M Cl2 at 668 K, which is an equilibrium mixture at this temperature. COCl2(g) = CO(g) + Cl2(g) a. When the temperature is increased and equilibrium is re-established, [COC12] = 0.18 M. Is the reaction endothermic or exothermic? How do you know? b. To the equilibrium mixture at 668 K, 0.25 M CO is added. Calculate the concentration of each gas at equilibrium.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...

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