**Equilibrium System Analysis**Consider the following chemical system at equilibrium:\[ \Delta H^\circ = 198 \text{ kJ}, \quad K_c = 2.90 \times 10^{-2} \, \text{ at } 1.15 \times 10^3 \text{ K} \]\[ 2\text{SO}_3(g) \rightleftharpoons 2\text{SO}_2(g) + \text{O}_2(g) \]### Scenario: Volume Increase at Constant TemperatureWhen the volume of the equilibrium system is suddenly increased, analyze the following aspects:1. **Value of \( K_c \):** - A. Increases - B. Decreases - C. Remains the same2. **Value of \( Q_c \) Relative to \( K_c \):** - A. Greater than \( K_c \) - B. Equal to \( K_c \) - C. Less than \( K_c \)3. **Reaction Direction:** - A. Runs in the forward direction to reestablish equilibrium. - B. Runs in the reverse direction to reestablish equilibrium. - C. Remains the same, it is already at equilibrium.4. **Number of Moles of \( \text{O}_2 \):** - A. Increase - B. Decrease - C. Remain the same**Instructions:** Choose the correct options for the above scenarios. After making your selections, click the "Submit Answer" button. You have 8 more attempts remaining for this group of questions.

The reaction given is, => 2 SO3 (g) -------> 2 SO2 (g) + O2 (g) Given : ΔHo = 198 KJ and Kc =…

Consider the following system at equilibrium where AH° = 198 kJ, and K. 2.90×10², at 1.15x10° K. 2S03(g)2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of K. A. increases. B. decreases. C. remains the same. The value of Q. A. is greater than K.. B. is equal to K C. is less than K. 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 O2 will: A. increase. B. decrease. C. remain the same.

Consider the following system at equilibrium where AH° = 198 kJ, and K. 2.90×10², at 1.15x10° K. 2S03(g)2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of K. A. increases. B. decreases. C. remains the same. The value of Q. A. is greater than K.. B. is equal to K C. is less than K. 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 O2 will: A. increase. B. decrease. C. 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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