he decomposition of NH₂HS NH4HS (8)NH, (g) + H₂S(g) an endothermic process. a. Using Le Chatelier's principle, explain how the equilibrium would be affected by increasing the temperature. shift left Oshift right Ono change b. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? Oshift left shift right Ono change c. If some additional NH3 is placed in the flask, how is the equilibrium affected? Oshift left shift right Ono change d. What will happen to the pressure of NH3 if some H₂S is removed from the flask? Oincrease

he decomposition of NH₂HS NH4HS (8)NH, (g) + H₂S(g) an endothermic process. a. Using Le Chatelier's principle, explain how the equilibrium would be affected by increasing the temperature. shift left Oshift right Ono change b. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? Oshift left shift right Ono change c. If some additional NH3 is placed in the flask, how is the equilibrium affected? Oshift left shift right Ono change d. What will happen to the pressure of NH3 if some H₂S is removed from the flask? Oincrease

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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If we represent the equilibrium as: 2 NO2(g) = N204(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
4. Name two ways in which a system at equilibrium can be disturbed.
Consider the following reaction and its equilibrium constant at some temperature. 2NH3(g) = N₂(g) + 3H₂(g) K₂=35 If the following concentrations are present initially: [NH3] = 0.10 M; [N₂] = 2.00 M; [H₂) = 2.00 M.. Which of the following is correct about the reaction? 1.The reaction is at equilibrium. 2.The reaction is not at equilibrium, it will shift to the left to reach equilibrium. 3.the reaction is not at equilibrium it will shift to the right to reach equilibrium.
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1.QuestionGiven the reaction at equilibrium: 2 SO2(g) + O2(g) <--> 2 SO3(g) + heat Which change will shift the equilibrium to the right? increasing the temperature increasing the pressure decreasing the amount of SO2(g) decreasing the amount of O2(g)
Write the equilibrium expression for 2NO(g) + 2H2(g) = N2(g) + 2H20(g). a. Ke = [H20]2 [N2] / [NO]² [H2]² O b. Kc [N2]/ [NO]2 [H2]? %3D O c. Ke [NO]? [H2]? / [H2O]² [N2] %3D
Consider the following equilibrium: 2 NH3(g) N2 (g) + 3 H2(g) Which of the following will happen when nitrogen gas (N₂) is added to the reaction mixture? --> The concentration of NH3 will decrease. The value of Keq will increase. The value of Keq will decrease. The concentration of H₂ will decrease.