What Percentage of PCl5 Will Decompose at 523K?

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The discussion revolves around calculating the percentage of PCl5 that decomposes at 523K given the equilibrium constant Kp of 0.500 for the reaction PCl5 (g) <-> PCl3 (g) + Cl2 (g). Participants emphasize the importance of understanding the definition of Kp to approach the problem effectively. The initial pressure of PCl5 is set at 0.100 atm, and the calculation involves determining the equilibrium concentrations of the products and reactants. Insight is provided on how to set up the equilibrium expression based on the given Kp value. Ultimately, the focus is on applying the equilibrium principles to find the percentage of PCl5 that decomposes.
rcrx
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For the reaction at 523K PCl5 (g) <-> PCl3 (g) + Cl2 (g) and Kp = 0.500

What percentage of PCl5(g) will decompose if 0.100 atm of PCl5(g) is placed in a closed vessel at 523K?

I am unsure of how to approach this problem, if anyone could give some insight I would greatly appreciate it.
 
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Look at your definition of Kp. All will become apparent.
 

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