Solving Equilibrium Problem: PCl5 <--> PCl3 + Cl2

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To solve the equilibrium problem involving the reaction PCl5 <--> PCl3 + Cl2, the initial moles of PCl5 are given as 0.40 mol, and the equilibrium moles of Cl2 are 0.25 mol. Using the stoichiometry of the reaction, the change in moles of PCl5 can be calculated, leading to the equilibrium moles of PCl3. The equilibrium concentrations are then determined by dividing the moles by the volume of the flask (10.0 L). Finally, the equilibrium constant Ke can be calculated using the formula Ke = [PCl3][Cl2]/[PCl5].
tornzaer
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Hi, I have no clue how to solve this problem:

Given that the initial n of PCl5 is 0.40 mol and the equilibrium n of Cl2 = 0.25 mol for the following equilibrium in a 10.0 L flask, find the Ke for these conditions.

PCl5(g) <-----> PCl3(g) + Cl2(g)


Thanks a lot of your help. :)
 
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