For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.140 at a certain temperature. A flask is charged...

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.140 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.

What are the equilibrium partial pressures of PCl3 , Cl2, and PCl5, respectively? Express your answers numerically in atmospheres with three digits after the decimal point, separated by commas.

Expert Solution

queen_honey_blossom answered 2 years ago

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.160 at a certain temperature. A flask is charged...

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 0.160 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. What are the equilibrium partial pressures of PCl3, Cl2, and PCl5? How will the following changes affect the mole fraction of chlorine gas, X Cl2, in the equilibrium mixture. X Cl2 increases when __________ X Cl2 decreases when _________ X Cl2 stays the same __________ Fill in the blanks...

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