Jen S.

asked • 02/16/21

At a certain temperature, an equilibrium mixture in a 1.00 L container consists of 0.00400 M PCl5(g), 0.100 M PCl3(g), and 0.200 M Cl2(g).

6.) At a certain temperature, an equilibrium mixture in a 1.00 L container consists of 0.00400 M PCl5(g), 0.100 M PCl3(g), and 0.200 M Cl2(g). (a) Calculate KC for PCl5(g) ⇌ PCl3(g) + Cl2(g); (b) To this mixture is added 0.100 mol of PCl3(g). Predict whether the new equilibrium concentrations will be higher than, lower than, or equal to the original equilibrium concentrations after the reaction returns to equilibrium; (c) Calculate the new equilibrium concentrations of the three gases. Are your answers consistent with your predictions?


8.) The volume of the container with the original equilibrium mixture in exercise 6 is doubled. (a) Calculate QC after the container changes in size but before any shift occurs; (b) Does the equilibrium shift? Which way? (c) What are the new equilibrium concentrations? Compare them with the original equilibrium concentrations.

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