Assigned problems _6 Answers - Chemistry 2080 Spring 2011...

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Chemistry 2080 Spring 2011 Problem Set #6 - due date: Friday March 18th at 2 pm Name:_____ KEY______ Lab TA Name:__________________ Lab Day/Time:______________________ 1) Phosphorus pentachloride decomposes at elevated temperatures: PCl 5 (g) PCl 3 (g) + Cl 2 (g) An equilibrium mixture at a certain temperature consists of 3.120 g of PCl 5 , 3.845 g of PCl 3 and 1.787 g of Cl 2 in a 1.00 L flask. If you add 1.418 g of Cl 2 , how will the equilibrium be affected? What will be the concentrations PCl 5 , PCl 3 , and Cl 2 when equilibrium is reestablished? __________________________________________________________________ First we need to calculate the value of the equilibrium constant, K c . To do this, we must convert the masses of compounds to moles and thence to molarities. The molar mass of PCl 5 is 208.239, of PCl 3 is 137.333, and of Cl 2 is 70.906 Thus 3.120 g of PCl 5 is (3.120 g/208.239 g/mol) = 0.01498 mol 3.845 g of PCl 3 is (3.845 g/137.333 g/mol) = 0.027998 mol and 1.787 g of Cl
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This note was uploaded on 03/28/2011 for the course CHEM 2080 taught by Professor Davis,f during the Spring '07 term at Cornell University (Engineering School).

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Assigned problems _6 Answers - Chemistry 2080 Spring 2011...

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