A student ran the following reaction in the laboratory at 545 K: COC12 (g) CO(g) + Cl₂ (g) When she introduced 0.604 moles of COC12 (9) into a 1.00 liter container, she found the equilibrium concentration of Cl₂ (g) to be 0.0302 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

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Chapter1: Chemical Foundations
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A student ran the following reaction in the laboratory at 545 K:
COC12 (g) CO(g) + Cl₂ (g)
When she introduced 0.604 moles of
COC12 (g) into a 1.00 liter container, she found the equilibrium concentration of
Cl₂ (g) to be 0.0302 M.
Calculate the equilibrium constant, Kc, she obtained for this reaction.
Kc =
Transcribed Image Text:A student ran the following reaction in the laboratory at 545 K: COC12 (g) CO(g) + Cl₂ (g) When she introduced 0.604 moles of COC12 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂ (g) to be 0.0302 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
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