3. A sealed vessel contains 0.25 M COC12, 0.11 M CO, and 0.11 M Cl, at 668 K, which is an equilibrium mixture at this temperature. COCI2(g) = CO(g) + Cl2(g) a. When the temperature is increased and equilibrium is re-established, [CoCl2] = 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.
3. A sealed vessel contains 0.25 M COC12, 0.11 M CO, and 0.11 M Cl, at 668 K, which is an equilibrium mixture at this temperature. COCI2(g) = CO(g) + Cl2(g) a. When the temperature is increased and equilibrium is re-established, [CoCl2] = 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.
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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