Consider the following system at equilibrium where AH° = 10.4 kJ, and Kc = 0.0180, at 698 K: 2HI(g) → H₂(g) + 12 (9) If the VOLUME on the equilibrium system is suddenly decreased at constant temperature: The value of Ke Oincreases Odecreases Oremains the same The value of Qc Ois greater than Ke Ois equal to Kc Ois 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 I2 will Oincrease Odecrease romain the came

Consider the following system at equilibrium where AH° = 10.4 kJ, and Kc = 0.0180, at 698 K: 2HI(g) → H₂(g) + 12 (9) If the VOLUME on the equilibrium system is suddenly decreased at constant temperature: The value of Ke Oincreases Odecreases Oremains the same The value of Qc Ois greater than Ke Ois equal to Kc Ois 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 I2 will Oincrease Odecrease romain the came

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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2. Explain how each of the following factors affects the amount of hydrogen gas present in an equilibrium mixture in the following reaction: 3 Fe(s) + 4 H,O(g) Fe;O4(s) + 4 H2(g) AH = - 150KJ 1) addition of a catalyst e) decreasing the volume
Consider the following equilibrium: 2NO, (g) = N,04 (g) AG° = - 5.4 kJ Now suppose a reaction vessel is filled with 8.21 atm of dinitrogen tetroxide (N,0,a) at 588. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,0, tend to rise or fall? '2 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,O, will tend to rise, can that 4. yes be changed to a tendency to fall by adding N0,? Similarly, if you said the no pressure of N,04 will tend to fall, can that be changed to a tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, 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 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.
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
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:
Equilibrium: 7. Write the equilibrium expression, K, for the following reactions: 2NH, (g) + CO2 (g) N,CH,0 (s) + H,0 (g) K= N2 (g) + 02 (g) 2 NO (g) K= 8. Consider the following reaction at equilibrium. 2S0, (g) 2S0, (g) + 02 (g) Predict the affect on equilibrium (will it shift left, shift right or no change?): a. Oxygen gas is removed: b. The volume is increased: c. The pressure is increased: d. SO, is added: e. SO, is added:
[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 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