Suppose a 250. mL flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) HCI(g) +CC14(g) The equilibrium constant K for this reaction is 3.83 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M

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Suppose a 250. mL. flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible:
Cl₂(g) + CHC1₂(g) → HCl(g) +CCl4 (g)
The equilibrium constant K for this reaction is 3.83 at the temperature of the flask.
Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places.
M
S
Transcribed Image Text:Suppose a 250. mL. flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HCl(g) +CCl4 (g) The equilibrium constant K for this reaction is 3.83 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M S
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