Question 26 4 pts Given the following equilibrium reaction, identify the effect each change will have as the reaction shifts to reestablish equilibrium. 2NO2 (g) N2O4 (g) AH = -55 kJ Decide if each change would cause the reaction to shift to favor reactants, products, or cause no change. Change Effect on Equilibrium Decrease in the temperature [Select] Decrease the volume [Select] Decrease in reactants [Select] Add a catalyst [Select] > > >

Question 26 4 pts Given the following equilibrium reaction, identify the effect each change will have as the reaction shifts to reestablish equilibrium. 2NO2 (g) N2O4 (g) AH = -55 kJ Decide if each change would cause the reaction to shift to favor reactants, products, or cause no change. Change Effect on Equilibrium Decrease in the temperature [Select] Decrease the volume [Select] Decrease in reactants [Select] Add a catalyst [Select] > > >

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 3RQ

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For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
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