Consider the following system at equilibrium where AH° = -87.9 kJ/mol, and K. = 83.3 , at 500 K.PCI3 (g) + Cl2 (g) =PCI5 (g)When 0.22 moles of PCI3 (g) are removed from the equilibrium system at constant temperature:The value of Keincrease.decrease.remain the same.The value of QcK..is greater thanis equal tois less thanThe reaction mustOrun in the forward direction to restablish equilibrium.Orun in the reverse direction to restablish equilibrium.Oremain the same. It is already at equilibrium.The concentration of Cl, willincrease.decrease.remain the same.

Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on chemical equilibrium. This principle states that when any system at equilibrium for a long period of time is subjected to a change in concentration, temperature, volume, or pressure the system changes to a new equilibrium, and this change partly counteracts the applied change.For the given equilibrium the expression for the equilibrium constant is given by: The value of the equilibrium constant is constant at a particular temperature and it does not change with the concentration of the reactants and product. The value of the equilibrium constant is changed on change with temperature. When we removed the product from equilibrium the reaction proceeds to the right side and the concentration of the products is increased and the effect of the change is cancelled. The value of Kc remains the same (as its value depends only on temperature and the temperature remains constant.). The value of Qc is less than Kc. (as the concentration of the product is decreased) The reaction must run in the forward direction to establish the equilibrium. (to cancel the effect of change) The concentration of Cl2 will decrease. (because the forward reaction occurs).

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Consider the following system at equilibrium where AH° = -87.9 kJ/mol, and K. = 83.3 , at 500 K. PCI3 (g) + Cl, (g) =PC!5 (g) When 0.22 moles of PCI5 (g) are removed from the equilibrium system at constant temperature: The value of K. increase. decrease. remain the same. The value of Qc Ke- is greater than is equal to is less than The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of Cl2 will increase. |decrease. remain the same.

Consider the following system at equilibrium where AH° = -87.9 kJ/mol, and K. = 83.3 , at 500 K. PCI3 (g) + Cl, (g) =PC!5 (g) When 0.22 moles of PCI5 (g) are removed from the equilibrium system at constant temperature: The value of K. increase. decrease. remain the same. The value of Qc Ke- is greater than is equal to is less than The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of Cl2 will increase. |decrease. remain the same.

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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