O Microsoft OneDrivecaching and lea X OWLV2 | Online teaching and lea X+now.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-takeConsider the following system at equilibrium where AH° = -198 kJ, and K. = 34.5 , at 1.15×10³ K:2 SO2 (g) + 02 (g)=2 SO3 (g)If the TEMPERATURE on the equilibrium system is suddenly decreasedThe value of K.A. IncreasesB. DecreasesC. Remains the sameThe value of QcA. Is greater than K.B. Is equal to KeC. 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 AnswerRetry Entire Group9 more group attempts remainingPreviousCEChp17fafi0f12insprt scdeleteho

Based on the change in the enthalpy for the equilibrium reaction, the change in enthalpy given is…

Consider the following system at equilibrium where AH° =-198 kJ, and K. = 34.5 , at 1.15×10° K: 2 SO2 (g) + 02 (g)=2 S03 (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 Ke 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.

Consider the following system at equilibrium where AH° =-198 kJ, and K. = 34.5 , at 1.15×10° K: 2 SO2 (g) + 02 (g)=2 S03 (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 Ke 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.

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...

See similar textbooks

Similar questions

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 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 system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc fill in the blank 1 A. increases. B. decreases. C. remains the same. The value of Q 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 reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The concentration of H2 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° = -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.
None
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.