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Suppose a 500.mL flask is filled with 0.90mol of Br2, 0.30mol of OCl2 and 1.5mol of...

Suppose a 500.mL flask is filled with 0.90mol of Br2, 0.30mol of OCl2 and 1.5mol of BrCl. The following reaction becomes possible: +Br2gOCl2g +BrOClgBrClg The equilibrium constant K for this reaction is 0.841 at the temperature of the flask. Calculate the equilibrium molarity of OCl2. Round your answer to two decimal places

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Answer #1

The balanced chemical equation is

Total volume

An ICE table is made

Initial number of moles 0.90 0.30 0 1.5
Change in number of moles -x -x +x +x
equilibrium number of moles
Equilibrium molarity (M)

The equilibrium constant

Rearrange above equation

Rearrange above equation

This is quadratic equation with solution

Negative value is discarded as concentration cannot be negative

The equilibrium concentration

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