Consider the following system at equilibrium where K. = 5.10×10-0 and AH° = 268 kJ/mol at 548 K. %3D NH,CI (s)=NH3 (g) + HCI (g) The production of NH3 (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). 3. decreasing the volume. 4. adding NH,Cl. 5. removing HCI .

Consider the following system at equilibrium where K. = 5.10×10-0 and AH° = 268 kJ/mol at 548 K. %3D NH,CI (s)=NH3 (g) + HCI (g) The production of NH3 (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). 3. decreasing the volume. 4. adding NH,Cl. 5. removing HCI .

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.
Ammonia can be synthesized according to the reaction: N2(g) + 3H2(g) = 2NH3(g), K = 5.3x10-5 at 725K. A 200.0L reaction container intially contains 1.27kg of N2 and 0.310kg of H2 at 725K. Assuming ideal gas behaviour, calculate the mass of NH3 (in g) present in the reaction at equilibrium. What is the percent yield under these conditions?
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 .
For the first one the options are increases, decreases, and remains the same.
Consider the following system at equilibrium where K. = 9.52x102 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CC14 (g) =2 CH,Ch (g) The production of CH,Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: |1. decreasing the temperature. | 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. v 4. adding CH,Cl . | 5. removing CCI4 .
For the equilibrium N2(g)+O2 <-->2NO(g), Kp = 0.0017 at 2300 K. At a given point, the partial pressures of the gases are PN2=PO2 = 0.660 atm and PNO= 0.0272atm. Which statment below is true? a. Q < K, so the reaction will continue to make more products. b. Q > K, so the reaction will consume products to make more reactants. c. Q = K, so the system is at equilibrium. d. The value of K will decrease until it is equal to Q. Show your work:
Kc = 0.76 at a given temperature for the reaction: 2 HI (g) = H2 (g) + l2 (g) . Consider the condition [HI] = 0.36 M and [H2] = [12] = 0.60 M. Which of the following statements is correct? a) The quotient Q > Kc. b) The reaction will shift to right to establish equilibrium. O a) only O b) only Both a) and b) are correct. neither a) nor b) is correct.
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:
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
A mixture of 0.422 M H,, 0.376 M I,, and 0.913 M HI is enclosed in a vessel and heated to 430 °C. H,(g) + 1,(g) = 2 HI(g) K. = 54.3 at 430 °C Calculate the equilibrium concentrations of each gas at 430 °C. [H,] = M L] = M [HI] = M