At a certain temperature and a total pressure of 1.2 atm, the partial pressures of an equilibrium mixture 2A(g) 2 B(g) are PA = 0.60 atm and PB = 0.60 atm. (a) Calculate the Kp for the reaction at this temperature. (b) If the total pressure were increased to 1.5 atm, what would be the partial pressures of A and B at equilibrium?
At a certain temperature and a total pressure of 1.2 atm, the partial pressures of an equilibrium mixture 2A(g) 2 B(g) are PA = 0.60 atm and PB = 0.60 atm. (a) Calculate the Kp for the reaction at this temperature. (b) If the total pressure were increased to 1.5 atm, what would be the partial pressures of A and B at equilibrium?
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter13: Chemical Equilibrium
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Problem 112CP: Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were...
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Transcribed Image Text:At a certain temperature and a total pressure of 1.2 atm, the partial pressures of an equilibrium mixture
2A(g) 2 B(g)
are PA = 0.60 atm and PB = 0.60 atm. (a) Calculate the Kp for the reaction at this temperature. (b)
If the total pressure were increased to 1.5 atm, what would be the partial pressures of A and B at
equilibrium?
Expert Solution
Step 1
Given data:
- The partial pressure of A at equilibrium = 0.60 atm
- The partial pressure of B at equilibrium = 0.60 atm
- Total pressure = 1.20 atm
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