21-2. Consider the following equilibrium. Which way will the system shift, if at all? How would thefollowing changes affect the partial pressures of each gas at the new equilibrium, if at all?How will the equilibrium constant change, if at all?a.PC13(g) +Cl2(g) + PCI5(g) AH = -56 kJShift(pPc13)(pcı2)(ppcis)KAddition of PCI3Removal of PC33Removal of Cl2Addition of Cl2Removal of PCI5Addition of PCI5Addition of He(g)Decrease container volumeIncrease container volumeIncrease temperatureDecrease temperature

Given reaction is: PCl3 (g) + Cl2 (g) → PCl5 (g) - 56.0 kJ So, the above reaction edothermic from…

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all? a. PCl3(8) Cl2(g) + PCI5(g) AH = -56 kJ Shift (prc13) (раз) (prcis) K Addition of PCl3 Removal of PCla Removal of Cl2 Addition of Cl2 Removal of PCI5 Addition of PCls Addition of He(g) Decrease container volume Increase container volume Increase temperature Decrease temperature

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all? a. PCl3(8) Cl2(g) + PCI5(g) AH = -56 kJ Shift (prc13) (раз) (prcis) K Addition of PCl3 Removal of PCla Removal of Cl2 Addition of Cl2 Removal of PCI5 Addition of PCls Addition of He(g) Decrease container volume Increase container volume Increase temperature Decrease temperature

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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