Consider the following system at equilibrium where AH= 92.7 kJ, and K. -1.80x104, at 298 K. NH,HS(s) NH(®) + H2S(g) When some moles of NH,HS(s) are added to the equilibrium system at constant temperature: The value of K. The value of Q. V K. 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 NH3 will

Consider the following system at equilibrium where AH= 92.7 kJ, and K. -1.80x104, at 298 K. NH,HS(s) NH(®) + H2S(g) When some moles of NH,HS(s) are added to the equilibrium system at constant temperature: The value of K. The value of Q. V K. 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 NH3 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...

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1. Industrially sulfuric acid is produced by reaction below at 800 K. SO2 (2)_ + O2(g) SO:(g) The reaction mixture is held at constant temperature of 800 K, and it reaches at equilibrium, with the composition below, what is the equilibrium constant at 800 K. (first balance the chemical equation above, show all the detail calculation and the equilibrium formula) Composition a) SO3,_ 4.9 x10-2 M, O2 , 3.3×10-3 M, and SO2 2.9×10-³M b) What is the equilibrium constant at 800 K, if the equilibrium concentration of SO2 is further decreased by 10% from what is given in (a)
Consider the following chemical equilibrium: CaCO; (s)= CaO ()+CO, (g) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature 7. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator.
10. At certain temperature, 0.80 mole of CO and 0.60 mole of Cl2 was introduced into an evacuated 2.00-liter container. The system was allowed to reach equilibrium at the new temperature. At equilibrium 0.40 mole COC)2 was present in the container. Calculate the equilibrium constant, Kc at this temperature. Co (g) + Cl2 (g) = cOCl2 (g) A. 10.0 В. О.1 С. 1.0 D. 2.5
CH,(g) + CCl,(g) 2CH,Cl,(g) When 0.40 moles of CC4(g) are added to the equilibrium system at constant temperature: The value of K. The value of Qc The reaction must Orun in the forward direction to restablish equilibrium. Oru run in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium.
Consider the following reaction: 2HF(g) ⟷H2(g) + F2(g) (K = 1.00 x10-2) Given 1.00 mole of HF(g), 0.500 mole of H2(g), and 0.750 mole of F2(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q, and the net direction to achieve equilibrium.
Consider the following chemical equilibrium: 4 NH, (g) +3 0, (g)=2N, (g) +6 H,Oo (g) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K_ = I
19. Given the following reaction: NH.CI (s) S NH3 (g) + HCI (g) AH= +42.1 kcal Suppose the above substances in the reaction are at equilibrium at 600 K in volume V and at pressure P. State whether the partial pressure of NH3 (g) will have increased, decreased, or remained the same in order to the equilibrium to be reestablished following the disturbances of the original system. Note that some solid remains in the flask at all times. Provide a one to two sentence explanation (a) The temperature of the system is increased (b) The volume of the system is increased (c) A quantity of gaseous NH3 is added. (d) A small quantity if NH4C1 is added.
4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) The value for the equilibrium constant for reaction 4.1 is Kc = 2.7 x 10-¹7 at some temperature T. A system initially has [N₂] = 0.0800 M and [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)
At a certain temperature, a 17.0-L container holds four gases in equilibrium. Their masses are 3.5 g SO3, 4.6 g SO₂, 11.9 g N₂, and 0.98 g N₂O. What is the value of the equilibrium constant at this temperature for the reaction of SO₂ with N₂O to form SO3 and N₂? Make sure you balance the reaction using the lowest whole-number coefficients. Kc =
Consider the following system at equilibrium where AH° = -87.9 kJ, and K. = 83.3, at 500 K. PC13(g) + Cl2(g) =PCI5(g) When 0.31 moles of Cl2(g) are removed from the equilibrium system at constant temperature: The value of K. increase. decrease. remain the same. The value of Qc K.. is greater than is equal to is less than 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 PC13 will increase. decrease. remain the same.
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.
ient/takeCovalentActivity.do?locator-assignment-take Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x102, at 1.15x10° K. 2S03(g) 2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value ofK. 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 reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of O, will: A. increase. B. decrease. C. remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Prev