63. Consider this reaction at equilibrium:MISSED THIS? Read Section 16.9; Watch KCV 16.9, IWE 16.14CO(g) + Cl2(g) = COCl2(g)Predict whether the reaction will shift left, shift right, or remainunchanged after each disturbance.a. COCl2 is added to the reaction mixture.b. Cl2 is added to the reaction mixture.c. COCl2 is removed from the reaction mixture.

Step 1:According to Le-chatelier's when system (reaction) is in equilibrium , if there in any change…

Answered: 63. Consider this reaction at…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 39A

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The decomposition of NH4HS, NH 4 HS( s )NH3( g )+ H 2 S( g ) is an endothermic process. Using Le Chatelier's principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
A mixture initially consisting of 2 mol CO and 2 mol H2 comes to equilibrium with methanol, CH3OH, as the product: CO(g)+2H2(g)CH3OH(g) At equilibrium, the mixture will contain which of the following? a less than 1 mol CH3OH b 1 mol CH3OH c more than 1 mol CH3OH but less than 2 mol d 2 mol CH3OH e more than 2 mol CH3OH
The decomposition of NH4HS NH4HS(s) NH3(g) + H2S(g) is an endothermic process. Using Le Chateliers principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?
Consider the reaction N2O4(g)2NO2(g). Draw a graph illustrating the changes of concentrations of N2O4 and NO2 as equilibrium is approached. Describe how the rates of the forward and reverse reactions change as the mixture approaches dynamic equilibrium. Why is this called a dynamic equilibrium?
Solid NH4HS decomposes by the following endothermic process: NH4HS(s) NH3(g) + H2S(g) a. What effect will adding more NH3(g) have on the equilibrium? b. What effect will adding more NH4HS(s) have on the equilibrium? c. What effect will increasing the volume of the container have on the equilibrium? d. What effect will decreasing the temperature have on the equilibrium?
The chapter opening photograph (page 670) showed how the cobalt(II) chloride equilibrium responded to temperature changes. (a) Look back at that photograph. Is the conversion of the red cation to the blue anion exothermic or endothermic? (b) If hydrochloric acid is added to the violet mixture of cobalt(II) ions shown below, the blue CoCl42 ion is favored. If water is then added to the mixture, a red solution favoring [Co(H2O)]2+ results. Explain these observations in terms of Le Chateliers principle. (c) How do these observations prove the reaction is reversible?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Decomposition of ammonium dichromate is shown in the designated series of photos. In a closed container this process reaches an equilibrium state. Write a balanced chemical equation for the equilibrium reaction. How is the equilibrium affected if more ammonium dichromate is added to the equilibrium system? more water vapor is added? more chromium(III) oxide is added? Decomposition of ammonium dichromate, for Question 4. Decomposition of (NH4)2Cr2O7. Orange, solid (NH4)2Cr2O7 (a) can be ignited by lighting a wick (b), which initiates decomposition (c) forming Cr2O3, the dark green solid in part (d), N2 gas, and water vapor. Energy is transferred to the surroundings by the process.
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
The formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2 NH3(g) 1. Does the reaction shift to the right or to the left, or does it remain unchanged, when extra H2 is added? (a) shift left (b) shift right (c)unchanged

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