Cobalt metal can be prepared by reducing cobalt(II) oxide with carbon monoxide. CoO(s) + CO(g) ⇌ Co(s) + CO2(g) Kc= 112.85 at 152.5°C What concentration of CO (in M) remains in an equilibrium mixture with [CO2] = 3.56 M?
Cobalt metal can be prepared by reducing cobalt(II) oxide with carbon monoxide. CoO(s) + CO(g) ⇌ Co(s) + CO2(g) Kc= 112.85 at 152.5°C What concentration of CO (in M) remains in an equilibrium mixture with [CO2] = 3.56 M?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.52QE: Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium...
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Cobalt metal can be prepared by reducing cobalt(II) oxide with carbon monoxide.
CoO(s) + CO(g) ⇌ Co(s) + CO2(g) Kc= 112.85 at 152.5°C
What concentration of CO (in M) remains in an equilibrium mixture with [CO2] = 3.56 M?
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