Consider the following system at equilibrium where AH° = 268 kJ, and K. = 5.10×10“, at 548 K. %3D NH,CI(s) NH3(g) + HCI(g) When some moles of NH,CI(s) are removed from the equilibrium system at constant temperature: The value of K The value of Q. ]K. The reaction must O run in the forward direction to restablish cquilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at cquilibrium. The concentration of NH, will

Consider the following system at equilibrium where AH° = 268 kJ, and K. = 5.10×10“, at 548 K. %3D NH,CI(s) NH3(g) + HCI(g) When some moles of NH,CI(s) are removed from the equilibrium system at constant temperature: The value of K The value of Q. ]K. The reaction must O run in the forward direction to restablish cquilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at cquilibrium. The concentration of NH, will

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 AH° = -16.1 kJ, and Kc = 154, at 298 K. 2NO(g) + Br₂(g)=2NOBr(g) When 0.11 moles of Br₂(g) are added to the equilibrium system at constant temperature: The value of Ke The value of Qc Ke. The reaction must O run in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of NO will
4HCN(I) + 5O2 (g) ---> 2H2 (g) + 4CO (g) + 2N2 (g) Calculate the value of K in this reaction at teh given temperature of 25 degrees C.
At room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold. HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). A.)Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔH<TΔS, ΔH=TΔS, ΔH>TΔS, or need more info). B.) Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔSuniv<0, ΔSuniv=0, ΔSuniv>0, or need more info).
Consider the following system at equilibrium where AH° = -18.8 kJ/mol, and Ke = 10.5 , at 350 K. 2 CH2CI2 (g)=CH4 (9) + CCI4 (9) When 0.34 moles of CH2CI2 (g) are removed from the equilibrium system at constant temperature: The value of K l The value of Qe The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of CH4 will
I2(g)+Br2(g) --> 2 IBr(g). Kc= 250. the system is charged with 0.0500 M of I2 and Br2. What value should the student obtain for the equilibrium concentration of IBr(g)?
2NO(g) + 2H₂(g) = 2H₂O(g) + N₂(g) K = 0.110 AH° = -707 kJ What is the equilibrium constant for the reaction when it is altered as below? H₂O(g) + N₂(g) ⇒ NO(g) + H₂(g) K' = [?] K' Enter
4NH3(g) +50₂(g) = 4NO(g) + 6H₂O(g) AH = -1000. kJ K = 1.35 The equilibrium concentrations are [NH3] = 0.20M, [02] = 0.90M, [H2O] = 1.34 M, and [NO] = [?] What is the equilibrium concentration of NO at 25 °C? [NO] M Enter
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 .
Consider the following system at equilibrium where AH° = 18.8 kJ, and K. = 9.52x102, at 350 K: CH4 (g) + CCl, (g) =2 CH,Cl, (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of K. |A. Increases B. Decreases C. Remains the same |A. Is greater than K. B. Is equal to K. C. Is less than K. The value of Qe JA. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl, will: A. Increase. B. Decrease. C. Remain the same.
4. Toluene, C;H8(1), is an important organic solvent. It is made industrially from methylcyclohexane, C,H14(g): C,H14(g) + heat ? 2C;H8(1) + 3H2(g) State three different changes to an equilibrium mixture of these reacting gases that would shift the reaction toward greater production of toluene. State and explain each change.
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.
A. Directions: Write equilibrium expression for the following chemical an equation: 1. N2 (g) + 3H2 (g) = 2NH3 2. Caco3 (s) = Cao (s) + CO2 (g) 3. 2Hg (1) + 02 (g) = 2H90 (s) 4. 2H,S (g) + 302 (g) = 2H20 (g) + 2s02 (g) 5. co, (g) + H2 (g) =CO2 (g) + H20 (1)