mediaTUTOR Effect of Volume Change on an Equilibrium |Consider the following system at equilibrium where AH° = 87.9 kJ, and Kc = 1.20x10-2, at 500 K.PCI5(9) PCl3(9) + Cl2(g)If the VOLUME of the equilibrium system is suddenly increased at constant temperature:The value of Ke:eThe value of Qc:The reaction must:A. increases.B. decreases.C. remains the same.QulamitA. is greater than Ke.B. is equal to KeC. is less than KeThe number of moles of Cl₂ will:A. run in the forward direction to reestablish equilibrium.B. run in the reverse direction to reestablish equilibrium.C. remain the same. It is already at equilibrium.[References]A. increase.B. decrease.C. remain the same.Show Approach Show Tutor StepsPreviousNext11:54 PM7/15/2022

Le Chatelier’s principle: When factors like concentration, pressure, temperature and Volume are…

edia UTOR Effect of Volume Change on an Equilibrium I Consider the following system at equilibrium where AH° = 87.9 kJ, and Kc = 1.20x10-2, at 500 K. PCI5(9) PCl3(g) + Cl2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of Ke: The value of Qc: The reaction must: C A. increases. B. decreases. C. remains the same. Submit A. is greater than Ke B. is equal to Ke C. is less than Ke The number of moles of Cl₂ will: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. [References] A. increase. B. decrease. C. remain the same. Show Approach Show Tutor Steps

edia UTOR Effect of Volume Change on an Equilibrium I Consider the following system at equilibrium where AH° = 87.9 kJ, and Kc = 1.20x10-2, at 500 K. PCI5(9) PCl3(g) + Cl2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of Ke: The value of Qc: The reaction must: C A. increases. B. decreases. C. remains the same. Submit A. is greater than Ke B. is equal to Ke C. is less than Ke The number of moles of Cl₂ will: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. [References] A. increase. B. decrease. C. remain the same. Show Approach Show Tutor Steps

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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Consider the following system at equilibrium where AH° = -87.9 k), and K. = 83.3, at 500 K. PCI3(g) + Cl2(g) PCI5(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of K. A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of Cl, will: A. increase. B. decrease. C. remain the same.
Consider the following system at equilibrium where Kc = 1.20E-2 and AH° = 87.9 kJ/mol at 500 K. PCI5(9) PC13(g) + Cl₂(g) The production of PCI3(g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. decreasing the pressure (by changing the volume). 3. decreasing the volume. 4. adding PC15- 5. adding Cl₂. CHEC
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Consider the following system at equilibrium where K = 1.20x10-2 and AH° = 87.9 kJ/mol at 500 K. PCI5 (9) — PCI3 (g) + Cl₂ (9) The production of PCI3 (g) is favored by: Indicate True (I) or False (F) for each of the following: 1. decreasing the temperature. ✓2. decreasing the pressure (by changing the volume). 3. increasing the volume. ✓4. adding PCI5. 5. adding Cl₂.
For the first one the options are increases, decreases, and remains the same.
Consider the following system at equilibrium where K. = 9.52x102 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CC14 (g) =2 CH,Ch (g) The production of CH,Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: |1. decreasing the temperature. | 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. v 4. adding CH,Cl . | 5. removing CCI4 .
Consider the following system at equilibrium where K. = 77.5 and AH° = -108 kJ/mol at 600 K. co (g) + Cl2 (g) = COCI2 (g) The production of COCI, (g) is favored by: Indicate True (I)_or False (E) for each of the following: 1. decreasing the temperature. v 2. increasing the pressure (by changing the volume). 3. decreasing the volume. v 4. removing COCI2 . v 5. removing Cl2 .
Why are these wrong?
At a certain temperature, the ?p for the decomposition of H2S is 0.770. H2S(g)↽−−⇀H2(g) + S(g) Initially, only H2S is present at a pressure of 0.268 bar in a closed container. What is the total pressure in the container at equilibrium? Ptotal= bar
Consider the following system at equilibrium where AH° = -87.9 kJ, and K. = 83.3, at 500 K. PC13(g) + Cl2(g) =PCI5(g) When 0.31 moles of Cl2(g) are removed from the equilibrium system at constant temperature: The value of K. increase. decrease. remain the same. The value of Qc K.. 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. Oremain the same. It is already at equilibrium. The concentration of PC13 will increase. decrease. remain the same.
Consider the following system at equilibrium where AH° = 18.8 kJ, and K. = 9.52x102, at 350 K: CH4 (g) + CCl, (g) =2 CH,Cl, (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of K. |A. Increases B. Decreases C. Remains the same |A. Is greater than K. B. Is equal to K. C. Is less than K. The value of Qe JA. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl, will: A. Increase. B. Decrease. C. Remain the same.
[References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 16.1 kJ, and Kc = 6.50 x 10-3, at 298 K: 2NOBr(g) 2NO(g) + Br₂(g) If the VOLUME on the equilibrium system is suddenly increased at constant temperature: The value of Ke Oincreases O decreases O remains the same The value of Qc O is greater than Ke O is equal to Ke O is less than K The reaction must run in the forward direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. Oremain the same. It is already at equilibrium. The number of moles of Br2 will O increase O decrease O remain the same Show Hint F5 6 H F6 & 7 KI F7 * 8 DII F8 ( 9 DD F9 ) O F10 P F11 Previous + Next Save and Exit F12 delete