14.40 For the synthesis of ammonia f0+N,(g) + 3H2(g) = 2NH3(g)lom 08 the equilibrium constant K, at 375°C is 1.2. Startingwith [H2lo = 0.76 M, [Nlo = 0.60 M, and [NH,lo =0.48 M, which gases will have increased in concen-tration and which will have decreased in concentra-%3D%3D|3Dtion when the mixture comes to equilibrium?

When rate of foroward reaction is equal to rate of backward reaction, then equilibrium is…

40 For the synthesis of ammonia f N2(g) + 3H2(g) 2NH,(g) the equilibrium constant K, at 375°C is 1.2. Starting slelwith (H2lo = 0.76 M, [N÷]o 0.60 M, and [NH,J, = 0.48 M, which gases will have increased in concen- tration and which will have decreased in concentra- tion when the mixture comes to equilibrium?2 %3D %3D

40 For the synthesis of ammonia f N2(g) + 3H2(g) 2NH,(g) the equilibrium constant K, at 375°C is 1.2. Starting slelwith (H2lo = 0.76 M, [N÷]o 0.60 M, and [NH,J, = 0.48 M, which gases will have increased in concen- tration and which will have decreased in concentra- tion when the mixture comes to equilibrium?2 %3D %3D

Chemistry

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ISBN:9781133611097

Author:Steven S. Zumdahl

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Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...

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At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced. Sb2S3(s)+3H2(g)2Sb(s)+3H2S(g) A vessel whose volume was 2.50 L was filled with 0.0100 mol of antimony(III) sulfide, Sb2S3, and 0.0100 mol H2. After the mixture came to equilibrium in the closed vessel at 440C, the gaseous mixture was removed, and the hydrogen sulfide was dissolved in water. Sufficient lead(II) ion was added to react completely with the H2S to precipitate lead(II) sulfide, PbS. If 1.029 g PbS was obtained, what is the value of Kc at 440C?
Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr. The reaction is 2NO(g)+Br2(g)2NOBr(g) a. Calculate the value of Kp. b. What would be the partial pressures of all species if NO and Br2, both at an initial partial pressure of 0.30 atm, were allowed to come to equilibrium at this temperature?
For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
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
At high temperatures, a dynamic equilibrium exists between carbon monoxide, carbon dioxide, and solid carbon. C(s)+CO2(g)2CO(g);H=172.5kJ At 850C, Kc is 0.153. a What is the value of Kp? b If the original reaction system consisted of just carbon and 1.50 atm of CO2, what are the pressures of CO2 and CO when equilibrium has been established? c How will the equilibrium pressure of CO change if the temperature is decreased?
Iodine chloride decomposes at high temperatures to iodine and chlorine gases. 2ICl(g)I2(g)+Cl2(g)Equilibrium is established at a certain temperature when the partial pressures of ICl, I2, and Cl2 are (in atm) 0.43, 0.16, and 0.27, respectively. (a) Calculate K. (b) If enough iodine condenses to decrease its partial pressure to 0.10 atm, in which direction will the reaction proceed? What is the partial pressure of iodine when equilibrium is reestablished?
At 25C. Kp = 5.3 105 for the reaction N2(g)+3H2(g)2NH3(g) When a certain partial pressure of NH3(g) is put into an otherwise empty rigid vessel at 25C, equilibrium is reached when 50.0% of the original ammonia has decomposed. What was the original partial pressure of ammonia before any decomposition occurred?
Consider the following system at equilibrium at 25C: PCl3(g)+Cl(g)PCl5(g)G=92.50KJ What will happen to the ratio of partial pressure of PCl5 to partial pressure of PCI3 if the temperature is raised? Explain completely.
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.

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