Consider the following system at equilibrium whereAH18.8 kJ andKc = 0.0952, at 350. K.CH4 (9) + CCl4 (9) ⇒ 2CH₂ Cl2 (g)If the VOLUME of the equilibrium system is suddenly decreased at constant temperature:The value of KcOincreasesOdecreasesOremains the sameThe value of QcOis greater than KeOis equal to KeOis less than KcThe reaction mustOrun 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 CC14 willOincreaseOdecreaseOremain the same

Consider the following system at equilibrium where AH = 18.8 kJ and Kc = 0.0952, at 350. K. CH4 (9) + CCl4 (9) ⇒ 2CH₂Cl₂ (9) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of Kc Oincreases Odecreases Oremains the same The value of Qc Ois greater than Kc Ois equal to Ke Ois less than K The reaction must Orun 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 CC14 will Oincrease Odecrease Oremain the same

Consider the following system at equilibrium where AH = 18.8 kJ and Kc = 0.0952, at 350. K. CH4 (9) + CCl4 (9) ⇒ 2CH₂Cl₂ (9) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of Kc Oincreases Odecreases Oremains the same The value of Qc Ois greater than Kc Ois equal to Ke Ois less than K The reaction must Orun 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 CC14 will Oincrease Odecrease Oremain 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

Consider the following equilibrium: N2 (g) + 3H, (g) – 2NH; (g) AG = - 34. kJ Now suppose a reaction vessel is filled with 7.31 atm of nitrogen (N,) and 7.58 atm of ammonia (NH,) at 1074. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding H,? In other words, if you said the pressure of NH, will tend to rise, can that yes be changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding H,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. atm Round your answer to 2 significant digits. O O
Consider the following system at equilibrium where AH° PC15 (9) PCl3 (g) + Cl₂ (g) O increases decreases O remains the same = If the temperature on the equilibrium system is suddenly increased: The value of K 87.9 kJ, and Ke 1.20 × 10-2, at 500 K: The concentration of Cl₂ will O increase decrease O remain the same The value of Q O is less than Kc O is greater than Kc O is equal to Kc The reaction must O run in the forward direction to reestablish equilibrium O run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium = Consider the wings All-179 The value of
Consider the following system at equilibrium where K. = 154 and AH° = -16.1 kJ/mol at 298 K. 2 NO (g) + Br2 (g) =2 NOBR (g) The production of NOB (g) is favored by: Indicate True (T) or False (F) for each of the following: v 1. increasing the temperature. v 2. increasing the pressure (by changing the volume). v 3. increasing the volume. v 4. removing NOB.. v 5. removing Br2 .
Consider the following system at equilibrium where AH° = -18.8 kJ/mol, and Kc = 10.5, at 350 K. 2 CH₂Cl₂ (9) CH4 (9) + CCI4 (9) When 0.33 moles of CH₂Cl₂ (g) are removed from the equilibrium system at constant temperature: The value of Kc The value of Qc Kc. 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 equilibrium. The concentration of CH4 will
Consider the following system at equilibrium where AH° = -111 kJ, and K = 0.159, at 723 K. %3D %3D N2(g) + 3H2(g) =2NH3(g) When 0.22 moles of H2(g) are added to the equilibrium system at constant temperature: The value of Kc The value of Qc. Kc. 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 equilibrium. The concentration of N2 will Submit Answer Retry Entire increase. roup attempts remaining decrease. remain the same.
reg # 3 [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. = 1.29 × 10-2, at 600 K: COC1₂ (g) CO(g) + Cl₂ (g) E 20 If the temperature on the equilibrium system is suddenly increased: The value of Ke D Oincreases Odecreases O remains the same The value of Qc Ols less than Ke Ois greater than K O is equal to Ke The reaction must Orun 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 Cl₂ will Oincrease Odecrease Oremain the same Submit Ans Show Hint $ 4 000 000 F4 R F % 5 T ry Entire Group Cengage Learning | Cengage Technical Support G A 6 9 more group attempts remaining MacBook Air Y H & 7 U * 00 8 ( 9 K O -0 ) F10 P 4) F11 Previous + 11 Next> Save and Ex A
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 equilibrium: 2NH₂ (g)-N₂ (g) + 3H₂(g) AG-34. KJ Now suppose a reaction vessel is filled with 4.85 atm of ammonia (NH3) a system: Under these conditions, will the pressure of H, tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of H, will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of H₂ 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. and 2.40 atm of hydrogen (H₂) at 658. °C. Answer the following questions about this Ⓒrise O fall yes no atm 10 10 X S
Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.
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
Consider the following system at equilibrium where AH° = 92.7 kJ, and K. =1.80x104, at 298 K. NH,HS(s) NH3(g) + H2S(g) When some moles of NH HS(s) are added to the equilibrium system at constant temperature: The value of Ke The value of Qel |Ke The reaction must Orun in the forward direction to restablısh equilibrium. Orun in the reverse direction to restablish equilibrium O remain the same. It is already at equilibrium. The concentration of NH3 will| Submit Answer Retry Entire Group No more group attempts remain
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