Consider the following system at equilibrium where K = 1.80x102 and AH = 10.4 kJ/mol at 698 K. 2 HI (9) H₂ (9) + 1₂ (9) The production of H₂ (g) Is favored by: Indicate True (T) or False (F) for each of the following: 1. Increasing the temperature. 2. Increasing the pressure (by changing the volume). 3. decreasing the volume. 4. removing HI. 5. removing I₂. Submit Answer Retry Entire Group 9 more group attempts remaining

Consider the following system at equilibrium where K = 1.80x102 and AH = 10.4 kJ/mol at 698 K. 2 HI (9) H₂ (9) + 1₂ (9) The production of H₂ (g) Is favored by: Indicate True (T) or False (F) for each of the following: 1. Increasing the temperature. 2. Increasing the pressure (by changing the volume). 3. decreasing the volume. 4. removing HI. 5. removing I₂. Submit Answer Retry Entire Group 9 more group attempts remaining

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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Consider the following system at equilibrium where H° = -198 kJ/mol, and Kc = 34.5 , at 1150 K.2 SO2 (g) + O2 (g) 2 SO3 (g)When 0.10 moles of SO3 (g) are added to the equilibrium system at constant temperature:The value of Kc The value of Qc Kc.The reaction must run in the forward direction to restablish equilibrium.run in the reverse direction to restablish equilibrium.remain the same. It is already at equilibrium. The concentration of O2 will
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Consider the following system at equilibrium where Kc = 34.5 and AH° = -198 kJ/mol at 1150 K. 2 SO₂ (g) + O₂ (g) 2 SO3 (g) The production of SO3 (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. decreasing the pressure (by changing the volume). 3. increasing the volume. 4. removing SO3. 5. removing 0₂.
Consider the following system at equilibrium where Kc = 55.6 and AH° = -10.4 kJ/mol at 698 K. H₂ (g) + I₂ (g) = 2 HI (g) The production of HI (g) is favored by: Indicate True (T) or False (F) for each of the following: ✓1. decreasing the temperature. ✓2. decreasing the pressure (by changing the volume). ✓3. decreasing the volume. ✓4. adding HI . ✓5. adding I₂.
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 Kc = 1.20E-2 and AH° = 87.9 kJ/mol at 500 K. PCI5(9) PC13(g) + Cl₂(g) The production of PCI3(g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. decreasing the pressure (by changing the volume). 3. decreasing the volume. 4. adding PC15- 5. adding Cl₂. CHEC
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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.