Consider the following system at equilibrium where Kc = 6.30 and AH° = 111 kJ/mol at 723 K. 2 NH3 (9) N₂ (g) + 3 H₂ (9) The production of N₂ (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. increasing the volume. 4. adding NH3. 5. adding H₂.

Consider the following system at equilibrium where Kc = 6.30 and AH° = 111 kJ/mol at 723 K. 2 NH3 (9) N₂ (g) + 3 H₂ (9) The production of N₂ (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. increasing the volume. 4. adding NH3. 5. adding H₂.

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 system at equilibrium where K, = 154 and AH° = -16.1 kJ/mol at 298 K. 2 NO (g) + Brz (g) =2 NOB (g) The production of NOB (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. increasing the volume. V 4. removing NOB . 5. adding Br2.
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
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 reaction SbH5 (g) SbH3 (g) + H2 (g) If 0.500 atm of SbH5 is introduced into an empty, closed container at 248oC and the system is allowed to reach equilibrium, 0.397 atm of SbH5 remains. Find Kp and Kc.
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
Consider the following system at equilibrium where K. 7.00x10-5 and AH° = 182 kJ/mol at 673 K. NH4I (s) = NH3 (g) + HI (g) The production of NH3 (g) is favored by: Indicate True (I) or False (F) for each of the following: 1. increasing the temperature. v 2. decreasing the pressure (by changing the volume). v 3. increasing the volume. v 4. adding NH4I . 5. removing HI .
Consider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 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. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S
Consider the following system at equilibrium where K. = 34.5 and AH° = -198 kJ/mol at 1150 K. 2 So, (g) + 02 (g) =2 S03 (g) The production of S03 (g) is favored by: Indicate True (T) or False (F) for each of the following: ]1. decreasing the temperature. v 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. 4. removing SO3 . 5. removing O2 -