[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 = 1.29 x 10-2, at 600 K: COC1₂ (g) CO(g) + Cl₂ (9) If the temperature on the equilibrium system is suddenly increased: The value of Ke Oincreases Odecreases O remains the same The value of Q Ols less than Ke Ois greater than Ke O is equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of Cl₂ will Oincrease decrease Oremain the same Submit Ans Show Hint ry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support Previous Next> Save and Ex

[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 = 1.29 x 10-2, at 600 K: COC1₂ (g) CO(g) + Cl₂ (9) If the temperature on the equilibrium system is suddenly increased: The value of Ke Oincreases Odecreases O remains the same The value of Q Ols less than Ke Ois greater than Ke O is equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of Cl₂ will Oincrease decrease Oremain the same Submit Ans Show Hint ry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support Previous Next> Save and Ex

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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FaceboOK [Review Topics] [References) Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° 268 kJ, and K. 5.10x106, at 548 K. %3D NH,CI(s) NH3(g) + HCI(g) When some moles of NH,CI(s) are removed from the equilibrium system at constant temperature: The value of K The value of Q. The reaction must O run in the forward direction to restablish equilibrium. O run in the reverse direction to restablish equilibrium. O remain the same. It is already at cquilibrium. The concentration of NH, will Retry Entire Group 1 more group attempt remaining Submit Answer
Chemistry > Consider the following system at equilibrium where AH° = -18.8 kJ, and Kc = 1.05 x 10¹, at 350 K: 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) If the temperature on the equilibrium system is suddenly increased: The value of Ke Oincreases decreases Oremains the same The value of Q Ois less than Ke Use the References to access imp is greater than Ke is equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of CC14 will increase decrease Oremain the same Submit Answer Retry Entire Group 7 more group attempts remaining
E D The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K. 80 PC13(g) + Cl₂(g) PCl5(g) If AH° for this reaction is -87.9 kJ, what is the value of Kp at 589 K? Kp Submit Answer 4 ? 000 000 R F DO LO % 5 Use the References to access important values if needed for this question. Retry Entire Group 7 more group attempts remaining T Cengage Learning Cengage Technical Support G < 6 Y H & 7 U J 8 I 9 K O 0 L P Previous Email Instructor Save and Exit + 11 Next { [ } ]
What is the equilibrium constarnt for the reaction at 645 K ? The change in enthalpy (AH) for a reaction is -34.4 kJ/mol . The equilibrium constant for the reaction is 1.8x10 at 298 K. Express your answer using two significant figures. V AE K-
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) When some moles of NH4Cl(s) are removed from the equilibrium system at constant temperature: The value of Ke Oincreases decreases Oremains the same The value of Qc Ois greater than Ke Ois equal to Ke Ois less than Kc The reaction must run in the forward direction to reestablish equilibrium. run in the reverse direction to reestablish equilibrium. remain the same. It is already at equilibrium. The number of moles of NH3 will Oincrease decrease Oremain the same
For the generic reaction shown, K = 0.355 (at 950 K). What can you conclude about AG and AG° in a reaction mixture for which Q = 0.205 at 950 K? 2AZ2(g) + Z2(g) = 2AZ3(g) Item equation/constant: AG = AG° + RT In Q Select one: O a. AG is positive and AG° is negative O b. AG and AG° are both negative O c. AG is negative and AG° is positive O d. AG and AG° are both positive
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 AH° = 10.4 kJ, and Kc = 1.80×10-2, at 698 K: 2HI(g) =H₂(g) + I₂(9) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to Kc C. Is less than Kc 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 I2 will: A. Increase. B. Decrease. C. Remain the same.
Hypothetically, the reaction H2 + 2IC1→ I2+ 2HC1 is first order in [H2] and second order in [ICI]. Based on the first fast step given below and the fact that the second step is the slow step, propose a second-step mechanism, and show that it conforms to the experimentally determined reaction order. Assume that [I2] does not affect the reaction rate. H2 + 2ICI → I2 + 2HC1 Fast: 2ICI → I2 + 2Cl Slow:
Which causes the system below, at equilibrium, to shift to the product side? 2C09) +10 > 2C0) , AH° = -283.3 kJ O Removing carbon monoxide O Increasing temperature O Adding carbon dioxide ORemoving oxygen O Increasing pressure
The conversion of glucose-6-phosphate to fructose-6-phosphate has a K'eg of 0.5. Based on that information, which of the following sets of changes in the terms of the Gibbs equation is correct? O AH°' negative AS" positive AG negative O AH positive AS' negative AG" positive O AH" positive AS" positive AG" negative O AH' negative AS' positive AG" positive
Give typed full explanation not a single word hand written otherwise leave it