A student ran the following reaction in the laboratory at 529 K: COC12 (9)CO(g) + Cl₂ (9) When she introduced 2.04 moles of COC1₂ (9) into a 1.00 liter container, she found the equilibrium concentration of COC12 (g) to be 2.00 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 529 K:
COCl₂(g) → CO(g) + Cl₂ (9)
When she introduced 2.04 moles of
COC1₂ (9) into a 1.00 liter container, she found the equilibrium concentration of
COC12 (g) to be 2.00 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 529 K: COCl₂(g) → CO(g) + Cl₂ (9) When she introduced 2.04 moles of COC1₂ (9) into a 1.00 liter container, she found the equilibrium concentration of COC12 (g) to be 2.00 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
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