We are being asked to calculate the equilibrium partial pressures for the given reaction:
PCl3(g)+Cl2(g) → PCl5(g) Kp = 0.100
When dealing with equilibrium and Kp:
• Kp → equilibrium units in terms of pressure
• Kp is an equilibrium expression:
▪ only gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the pressures in the equilibrium expression
What are the equilibrium partial pressures of PCl3 , Cl2, and PCl5, respectively?
For the exothermic reaction PCl3(g)+Cl2(g) → PCl5(g) Kp = 0.100 at a certain temperature.
A flask is charged with 0.500 atm PCl3, 0.500 atm Cl2, and 0.300 atm PCl5 at this temperature.
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