Phosphorus pentachloride decomposes at high temperatures. An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a Question Content AreaWhat will the concentration of PCl5 be when equilibrium is reestablished after addition of 1.31 g Cl2?
Phosphorus pentachloride decomposes at high temperatures. An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a Question Content AreaWhat will the concentration of PCl5 be when equilibrium is reestablished after addition of 1.31 g Cl2?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 43GQ: Phosphorus pentachloride decomposes at elevated temperatures. PCl5(g) PCl3(g) + Cl2(g) An...
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Question
Phosphorus pentachloride decomposes at high temperatures.
An equilibrium mixture at some temperature consists of
3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask.
a
Question Content Area
What will the concentration of PCl5 be when equilibrium is reestablished after addition of 1.31 g Cl2?
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