-198 kJ, and K = 34.5, at 1.15 × 10³ K:Consider the following system at equilibrium where AH° = -198 kJ, and Ke2SO2(g) + O2(g)=2SO3 (9)If the temperature on the equilibrium system is suddenly decreased:The value of KO increasesO decreasesOremains the sameThe value of QcO is less than KcO is greater than KcO is equal to KThe reaction mustOrun 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 increaseOdecreaseO remain the samePreviousNext

For the given reaction2SO2(g)+O2(g)⇌2SO3(g) The value of ΔH0 = -198 KJ.The negative value of ΔH0…

Answered: -198 kJ, and K = 34.5, at 1.15 × 10³ K:…

Chemistry

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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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5 [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 × 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 T The value of Q O is less than Ke O is greater than K O is equal to Kc 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 O F5 Show Hint A 6 F6 & 7 U K F7 * 8 DII F8 ( 9 F9 ) O F10 P Previous F11 + Next Save and Exit F12 delete
Olawiany Tepical Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 108 kJ, and K. = 1.29×102 at 600 K: COC,(g) CO(g) + C(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 Cl, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining Previ 50 hp
Consider the following system at equilibrium where Kc = 154 and H° = -16.1 kJ/mol at 298 K. 2 NO (g) + Br2 (g) 2 NOBr (g) The production of NOBr (g) is favored by:Indicate True (T) or False (F) for each of the following: ___decreasing the temperature. ___decreasing the pressure (by changing the volume). ___decreasing the volume. ___removing NOBr . ___adding Br2 .
Consider the following system at equilibrium where Kc = 1.20×10-2 and H° = 87.9 kJ/mol at 500 K.PCl5 (g) PCl3 (g) + Cl2 (g)The production of PCl3 (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. increasing the volume. 4. removing PCl5 . 5. removing Cl2 .
Consider the following system at equilibrium where Ho = 18.8 kJ, and Kc = 9.52E-2, at 350 K: CH4(g) + CCl4(g) 2 CH2Cl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: whats the value of Kc The value of Q The reaction must
[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH=-108 kJ, and K. 77.5, at 600 K. CO(g) + C,(g) COCI,(g) When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish cquilibrium. O remain the same. It is already at cquilibrium. The concentration of CO will Submit Answer Retry Entire Group 1 more group attempt remaining
Consider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S
Consider the following system at equilibrium where AH° = 92.7 kJ, and K. = 1.80×10-4, at 298 K. NH,HS(s)NH3(g) + H2S(g) When some moles of NH,HS(s) are removed from the equilibrium system at constant temperature: The value of K. The value of Qe |K- 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 NH3 will
Consider the following system at equilibrium where AH = 268 kJ and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) NH3(g) + HCl(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: decreasing the pressure (by changing the volume): increasing the volume: adding NH4Cl: adding HCl:
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.
what is the answer?
[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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