Problem 4 Review I Cc For the reaction 2CO (g) +02(g) = 2CO 2 (g ) , the equilibrium concentrations at a certain temperature are [CO2] = 0.10 mol/L, [02] = 1.7x102 mol/L, [CO] - 2.4x102 mol/L. Part B What is the value of Kat this temperature? Express your answer using two significant figures. ΑΣφ ? K = 25 Previous Answers Request Answer Submit x Incorrect; Try Again; 5 attempts remaining Part C Are reactants or products favored? P Pearson 2019 Pearson Education Inc. All rights reserved. | Terms of UseI Privacy Policy Permissions Contact Us Copyright

Problem 4 Review I Cc For the reaction 2CO (g) +02(g) = 2CO 2 (g ) , the equilibrium concentrations at a certain temperature are [CO2] = 0.10 mol/L, [02] = 1.7x102 mol/L, [CO] - 2.4x102 mol/L. Part B What is the value of Kat this temperature? Express your answer using two significant figures. ΑΣφ ? K = 25 Previous Answers Request Answer Submit x Incorrect; Try Again; 5 attempts remaining Part C Are reactants or products favored? P Pearson 2019 Pearson Education Inc. All rights reserved. | Terms of UseI Privacy Policy Permissions Contact Us Copyright

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 3RQ: Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105...

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At 2000 K, experiments show that the equilibrium constant for the formation of water is 1.6 1010. 2H2(g) + O2(g) 2H2O(g) Calculate the equilibrium constant at the same temperature for H2(g)+12O2(g) H2O(g)
Calculate the number of moles of HI that are at equilibrium with 1.25 mol of H2 and 1.25 mol of I2 in a 5.00-L flask at 44 C. H2+I22HI at Kc=50.2 at 448 C
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Le Chteliers principle is stated (Section 12-7) as follows: If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change. The systemN2(g)+3H2(g)2NH3(g) is used as an example in which the addition of nitrogen gas at equilibrium results in a decrease in H2 concentration and an increase in NH3, concentration. In the experiment the volume is assumed to be constant. On the other hand, if N2 is added to the reaction system in a container with a piston so that the pressure can be held constant, the amount o f NH3 actually could decrease, and the concentration of H2 would increase as equilibrium is reestablished. Explain how this can happen. Also, if you consider this same system at equilibrium, the addition of an inert gas. holding the pressure constant, does affect the equilibrium position. Explain why the addition of an inert gas to this system in a rigid container does not affect the equilibrium position.
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to each equilibrium? SO2CI2(g)SO2(g)+CI2(g) [SO2CI2]=0.12M,[CI2]=0.16M and [SO2]=0.050M. KC for the reaction is 0.078.
Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 2NO(g)N2(g)+O2(g)K=11031 For each reaction, assume some quantities of the reactants were placed in separate containers and allowed to come to equilibrium. Describe the relative amounts of reactants and products that would be present at equilibrium. At equilibrium, which is faster, the forward or reverse reaction in each case?
What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm? Cl2(g)+Br2(g)2BrCl(g)KP=4.7102
For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
7-41 The equilibrium constant at 1127°C for the following endothermic reaction is 571: If the mixture is at equilibrium, what happens to K if we: (a) Add some H2S? (b) Add some H2? (c) Lower the temperature to 1000°C?
Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?