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1.100 mol phosphorus pentachloride, PCl5 were placed in an empty, sealed, 2.00 L container at room...

1.100 mol phosphorus pentachloride, PCl5 were placed in an empty, sealed, 2.00 L container at room temperature, when PCl5 is a solid. Then temperature was raised to 250oC, all the chemical evaporated, and it was found that 45% of it (by mass) decomposed according to the equation: PCl5(g)  PCl3(g) + Cl2(g)

(a) What are the equilibrium molar concentrations of all three chemical compounds involved?

(b) What is the equilibrium constant K for that rxn?

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