Consider the following system at equilibrium where AH° = 92.7 kJ, and K. =1.80×10-4, at 298 K.NH,HS(s)NH3(g) + H2S(g)When some moles of NH,HS(s) are removed from the equilibrium system atconstant temperature:The value of K.The value of Qe|K-The reaction mustOrun 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 NH3 will

Answered: Image /qna-images/answer/e87b4f65-cebd-40a4-8840-2f9f9c5d6036.jpg

Consider the following system at equilibrium where AH° = 92.7 kJ, and K. = 1.80×104, at 298 K. NH,HS(s)=NH3(g) + H2S(g) When some moles of NH,HS(s) are removed from the equilibrium system at constant temperature: The value of K. The value of Qe [ |Kc- The reaction must Orun 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 NH3 wil |

Consider the following system at equilibrium where AH° = 92.7 kJ, and K. = 1.80×104, at 298 K. NH,HS(s)=NH3(g) + H2S(g) When some moles of NH,HS(s) are removed from the equilibrium system at constant temperature: The value of K. The value of Qe [ |Kc- The reaction must Orun 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 NH3 wil |

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

The decomposition of HI at low temperature was studied by injecting 2.50 mol of HI into a 10.32-L vessel at 25℃. What is [H2] at equilibrium for the reaction 2HI(g) H2(g) + I2(g); Kc = 1.2610-3 ?
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.
The equilibrium constant, Kp, describes the ratio of product and reactant concentrations at equilibrium in terms of partial pressures. Consider the reaction below which has K, of 870 at 25 °C. H;(g) + 1,(g) 2HI(g) (a) Determine the numbers of moles of:- (i) HI formed when H2 = 0.5 moles and I; = 0.5 moles (ii) I2 formed when H2 = 0.5 moles and HI = 1.5 moles
19
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?
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
For the first one the options are increases, decreases, and remains the same.
At a certain temperature, Keq = 135.5 for the following equilibrium: SO2(g) + NO2(g) <===> NO(g) + SO3(g) Suppose a reaction vessel at this temperature contained these three gases at the following concentrations: [SO2] = 0.00250 M, [NO2] = 0.00350 M, [NO] = 0.0250 M, [SO3] = 0.0400 M. a)Determine Qeq for the system. (b)Is the system at equilibrium? If it is not, indicate the direction toward which the system will move to reach equilibrium.
Consider the following system at equilibrium where AH° = 92.7 kJ, and K. =1.80x104, at 298 K. NH,HS(s) NH3(g) + H2S(g) When some moles of NH HS(s) are added to the equilibrium system at constant temperature: The value of Ke The value of Qel |Ke The reaction must Orun in the forward direction to restablısh equilibrium. Orun in the reverse direction to restablish equilibrium O remain the same. It is already at equilibrium. The concentration of NH3 will| Submit Answer Retry Entire Group No more group attempts remain
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.