Suppose a 250. mL flask is filled with 1.2 mol of CHCI,, 0.10 mol of HCl and 1.7 mol of CCl. The following reaction becomes possible: Cl, (g) + CHCI, (g) - HCI(g) +CCl,(g) The equilibrium constant K for this reaction is 5.74 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places.

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Suppose a 250. mL flask is filled with 1.2 mol of CHCI,, 0.10 mol of HCl and 1.7 mol of CCl,. The following reaction becomes possible:
Cl, (g) +CHCI, (g) - HC1(g)+CCl,(g)
The equilibrium constant K for this reaction is 5.74 at the temperature of the flask.
Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places.
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dlo
OM
Ar
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Transcribed Image Text:Suppose a 250. mL flask is filled with 1.2 mol of CHCI,, 0.10 mol of HCl and 1.7 mol of CCl,. The following reaction becomes possible: Cl, (g) +CHCI, (g) - HC1(g)+CCl,(g) The equilibrium constant K for this reaction is 5.74 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. G dlo OM Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use| Privacy Center | Accessibility
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