Consider the following system at equilibrium where AH° = 198 kJ, and Kc = 0.0290, at 1150 K: 2SO3(g)2SO2(g) + O2(g) If the VOLUME on the equilibrium system is suddenly decreased at constant temperature: The value of Ke O increases O decreases O remains the same The value of Qc Ois greater than Ke O is equal to Ke O is less than Ke The reaction must Orun in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The number of moles of O2 will O increase decrease O remain the same Previous Next

Consider the following system at equilibrium where AH° = 198 kJ, and Kc = 0.0290, at 1150 K: 2SO3(g)2SO2(g) + O2(g) If the VOLUME on the equilibrium system is suddenly decreased at constant temperature: The value of Ke O increases O decreases O remains the same The value of Qc Ois greater than Ke O is equal to Ke O is less than Ke The reaction must Orun in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The number of moles of O2 will O increase decrease O remain the same 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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To manufacture S03 with the reaction 2S02(g) + 02 - > 2S03(g) A H° = -99 kJ, one way to increase the equilibrium S03 would be to O decrease oxygen O decrease SO2 increase pressure increase temperature
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
Consider the following system at equilibrium where K, = 154 and AH° = -16.1 kJ/mol at 298 K. 2 NO (g) + Brz (g) =2 NOB (g) The production of NOB (g) is favored by: Indicate True (T) or False (F) for each of the following; | 1. increasing the temperature. 2. increasing the pressure (by changing the volume). | 3. increasing the volume. V 4. removing NOB . 5. adding Br2.
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 H° = -18.8 kJ, and Kc = 10.5, at 350 K:2CH2Cl2(g) CH4(g) + CCl4(g)If the TEMPERATURE on the equilibrium system is suddenly increased: The value of Kc fill in the blank 1 A. Increases B. Decreases C. Remains the same The value of Qc fill in the blank 2 A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: fill in the blank 3 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 CCl4 will: fill in the blank 4 A. Increase. B. Decrease. C. Remain the same.
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 = 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 H° = -18.8 kJ, and Kc = 10.5, at 350 K:2CH2Cl2(g) CH4(g) + CCl4(g)If the TEMPERATURE on the equilibrium system is suddenly increased: The value of Kc fill in the blank 1 A. Increases B. Decreases C. Remains the same The value of Qc fill in the blank 2 A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: fill in the blank 3 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 CCl4 will: fill in the blank 4 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
Consider the following equilibrium: 2NOCI (g) - 2NO (g) + Cl, (g) AG-41. kJ Now suppose a reaction vessel is filed with 4.69 atm of nitrosyl chloride (NOCI) and 4.34 atm of chlorine (CI,) at 641. "C. Answer the following questions about this system: rise Under these conditions, will the pressure of NOCI tend to rise or fall? O fall ? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fal by adding NO? Similarly, if you said the pressure of NOCI wil tend to fall, can that be changed to a tendency to rise by adding NO? O yes O no Ir you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits.