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At a certain temperature the equilibrium constant Kp = .132 for the reaction:PCl5(g) <--> PCl3(g) + Cl2(g)At equilibrium, the partial pressures of both PCl5 and PCl3 are 100 mmHg. What is the total pressure of the equilibrium system in mmHg?Here is what I got; [PCl3][Cl2]/[PCl5] = .132 and the partial pressures should be equal to their molar fractions. So [Cl2]/ = .132. this is only possible if Cl2 has a pressure of .132 mmHg which is not an answer. Something tells me I'm setting this up wrong. Thanks for any advice...
you have to convert mmHg to atm (or bar).
you need to convert mmHg to atmospheres so that the ideal gas constant will be valid:
Quote from: Shipwreck on March 28, 2014, 10:07:00 AMyou need to convert mmHg to atmospheres so that the ideal gas constant will be valid:You can express ideal gas constant in whatever units you want, including mmHg.
atm (standard state) pressure units
Quote from: Shipwreck on March 28, 2014, 01:27:39 PMatm (standard state) pressure unitshttp://goldbook.iupac.org/S05921.html1 bar (105 Pa) is the standard state since 1982.
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