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- Sep 29, 2004
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Hey guys, I've got a question:
I'm given that Keq 96.2 at 450C for P(Cl5) (aq) --> P(Cl3) (aq) + Cl2 (g) and that the equilibrium concentration of Cl2 = 3.50M and P(Cl5) = 3.50M. The question wants me to figure out what the equilibrium concentration of P(Cl3) is. It's actually a fairly simple problem to solve, but I'm having conceptual problems understanding the context of the problem. I don't understand how Cl2 can have a different concentration than PCl3, since these products both form at a 1:1 ratio. From what I understand, for every 1 mol of P(Cl5) that dissociates in the solution, you get 1 mol of P(Cl3) and 1 mol of Cl2. Therefore, in a conceptual sense, I thought that the concentration of Cl2 (3.50M) would have to equal the concentration of P(Cl3). But this is not the case, according to the solution that goes through the Keq = product/reactant calculation method. So can someone tell me where I'm going wrong in my thinking?
I'm given that Keq 96.2 at 450C for P(Cl5) (aq) --> P(Cl3) (aq) + Cl2 (g) and that the equilibrium concentration of Cl2 = 3.50M and P(Cl5) = 3.50M. The question wants me to figure out what the equilibrium concentration of P(Cl3) is. It's actually a fairly simple problem to solve, but I'm having conceptual problems understanding the context of the problem. I don't understand how Cl2 can have a different concentration than PCl3, since these products both form at a 1:1 ratio. From what I understand, for every 1 mol of P(Cl5) that dissociates in the solution, you get 1 mol of P(Cl3) and 1 mol of Cl2. Therefore, in a conceptual sense, I thought that the concentration of Cl2 (3.50M) would have to equal the concentration of P(Cl3). But this is not the case, according to the solution that goes through the Keq = product/reactant calculation method. So can someone tell me where I'm going wrong in my thinking?