Consider the following system at equilibrium whereAH° = 268 kJ, andKc = 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 KeOincreasesdecreasesOremains the sameThe value of QcOis greater than KeOis equal to KeOis less than KcThe reaction mustrun 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 willOincreasedecreaseOremain the same

Consider the following system at equilibrium where AH° 268 kJ, and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) → NH3 (9)+ HCl(9) When some moles of NH4Cl(s) are removed from the equilibrium system at constant temperature: The value of Ke Oincreases Odecreases Oremains the same The value of Qc Ois greater than Ke Ois equal to Ke is less than Ke 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 NH3 will increase Odecrease Oremain the same

Consider the following system at equilibrium where AH° 268 kJ, and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) → NH3 (9)+ HCl(9) When some moles of NH4Cl(s) are removed from the equilibrium system at constant temperature: The value of Ke Oincreases Odecreases Oremains the same The value of Qc Ois greater than Ke Ois equal to Ke is less than Ke 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 NH3 will increase 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

10:25 1 4 7 +/- ||| For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25 °C, it is found that the partial pressure of C is 0.280 atm. What is AG° for this reaction? (R = 8.314 J/mol K). 2 5 Question 7 of 15 8 kJ/mol 6 9 * 10% 0 Submit Periodic Table X x 100
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
H2(g) + I2(g) 2 HI(g) AH=120 kJ e) In which direction will the equilibrium shift (for the first reaction) when (i) HI(g) is removed, (ii) the temperature is decreased, (ii) the volume of the reaction system is increased, (ii) H2(g) is added?
8:57 Question 6 of 25 Submit Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.2 mol CH4, 2.8 mol H2S, 0.63 mol CS2, and 0.042 mol H2 at 93.0 °C. What are the values of Kc and Kp for the reaction at this temperature? CH.(g) + 2 H;S(g) =CS2(s) + 4 H2(g) 1 2 Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms. Kc = [0.042] 5 RESET [1.2] [2.8] [0.63] [0.042] [0.24] [0.56] [0.13] [0.0084] 2[2.8] [2.8]? 2[0.56] [0.56]? 4[0.042] [0.042]* 4[0.0084] [0.0084]* 0.063 16 6.6 x 10-8 1.5 x 107 Tap here or pull up for additional resources
Do 6-10.
Consider the following chemical reaction: C3H8 + 5 O2 <==> 3 CO2 + 4 H2O This reaction was determined to have a Kp = 2.00 * 103 at a temperature of 20 °C . What is the value of Kc for this reaction? (Please provide your answer to 3 significant figures)
[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
For the following equilibrium system, K = 1.39x10-11 at 298 K. F (aq) + H₂O (1) HF (aq) + OH- (aq) Assuming that you start with just F, and that no HF or OH is initially present, which of the following best describes the equilibrium system? O The forward reaction is favored at equilibrium. O The reverse reaction is favored at equilibrium. O Appreciable quantities of all species are present at equilibrium.
Consider the following system at equilibrium where ΔΗ° - 111 kJ, and == Kc = 0.159, at 7.23 × 10² K: N₂(g) + 3H₂ (g) — 2NH3 (g) If the temperature on the equilibrium system is suddenly decreased: The value of Kc Oincreases Odecreases Oremains the same The value of Qc is less than Ke Ois greater than Kc Ois 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 H₂ will Oincrease Odecrease Oremain the same
1-3