5[References]Use the References to access important values if needed for this question.Consider the following system at equilibrium where AH = -198 kJ, andKc = 34.5, at 1.15 × 10³ K:2SO2(g) + O2(g) = 2SO3(g)If the temperature on the equilibrium system is suddenly decreased:The value of KeO increasesOdecreasesO remains the sameTThe value of QO is less than KeO is greater than KO is equal to KcThe reaction mustO run in the forward direction to reestablish equilibriumOrun in the reverse direction to reestablish equilibriumO remain in the current position, since it is already at equilibriumThe concentration of O2 willO increaseO decreaseO remain the sameOF5Show HintA6F6&7UKF7*8DIIF8(9F9)OF10PPreviousF11+NextSave and ExitF12delete

Given eqm rxn: 2SO2(g) + O2 (g) <=> 2SO3(g) Kc = 34.5 & ∆H° = -198 kJ i.e an exothermic…

[References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = -198 kJ, and Kc = 34.5, at 1.15 x 10³ K: 2SO2(g) + O2(g) = 2SO3(g) If the temperature on the equilibrium system is suddenly decreased: The value of Ke O increases Odecreases O remains the same The value of Qc O is less than Ke Ois greater than Ke O is equal to Ke The reaction must O run in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of O2 will O increase O decrease O remain the same Show Hint Previous Next>

[References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = -198 kJ, and Kc = 34.5, at 1.15 x 10³ K: 2SO2(g) + O2(g) = 2SO3(g) If the temperature on the equilibrium system is suddenly decreased: The value of Ke O increases Odecreases O remains the same The value of Qc O is less than Ke Ois greater than Ke O is equal to Ke The reaction must O run in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of O2 will O increase O decrease O remain the same Show Hint Previous Next>

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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References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 198 kJ, and K, = 2.90x10, at 1150 K: 2SO3(g) =2502(g) + O2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: 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 restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of O, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Previc 50 hp ins ort sc delets 40
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[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
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