42. Assume the reaction: A-2B goes to equilibrium and further assume that the data belowrepresent the progress of reaction starting with only molecules of A present at time zero. Allchemicals are in the same phase. The approximate numerical value of the equilibrium constant,Kc is:a) 0 b) between 0.0 and 1.0 c)between 1.01 and 3.0 d) between 3.01 and 6.0d) none of the above

To determine the equilibrium constant Kc for the reaction A→2B, we can use the equation:Kc =…

Answered: 42. Assume the reaction: A-2B goes to…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 4ALQ: Given the reaction A+BC+D, consider the following situations: a. You have 1.3 M A and 0.8 M B...

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. Ammonia. a very important industrial chemical. is produced by the direct combination of the following elements under carefully controlled conditions: N2(g)+3H2(g)2NH3(g)Suppose. in an experiment, that the reaction mixture is analyzed after equilibrium is reached, and it is found, at a particular temperature. that [NH3]=0.25M,[H2]=3.4103M, and [N2]=5.3105M. Calculate the value of K at this temperature.
Given the reactionA(g)+B(g)C(g)+D(g), consider the following situations: i. You have 1.3 M A and 0.8 M B initially. ii. You have 1.3 M A, 0.8 M B. and 0.2 M C initially. iii. You have 2.0 M A and 0.8 M B initially. Order the preceding situations in terms. of increasing equilibrium concentration of D. Explain your order. Then give the order in terms of increasing equilibrium concentration of B and explain.
Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?
Given the reaction A+BC+D, consider the following situations: a. You have 1.3 M A and 0.8 M B initially. b. You have 1.3 M A, 0.8 M B, and 0.2 M C initially. c. You have 2.0 M A and 0.8 M B initially. Order the preceding situations in terms of increasing equilibrium concentration of D and explain your order. Give the order in terms of increasing equilibrium concentration of B and explain.
Chemical Equilibrium I Part 1: You run the chemical reaction C(aq)+D(aq)2E(aq) at 25C. The equilibrium constant Kc for the reaction at this temperature is 2.0. a Write the equilibrium-constant expression for the reaction. b Can you come up with some possible concentrations of C, D, and E that you might observe when the reaction has reached equilibrium at 25C? What are these values? c A student says that only a very limited number of concentrations for C, D, and E are possible at equilibrium. Is this true? State why you think this is true or is not true. d If you start with 1.0 M concentrations of both C and D and allow the reaction to come to equilibrium, would you expect the concentration of C to have decreased to zero? If not, what would you expect for the concentration of C? (An approximate value is fine.) Part 2: Consider the reaction A(aq)F(aq)+G(aq), whose equilibrium constant is 1.0 105 at 20C. For each of the situations described below, indicate whether any reaction occurs. If reaction does occur, then indicate the direction of that reaction and describe how the concentrations of A, B, F, and G change during this reaction. a A(aq) and B(aq) are mixed together in a container. b F(aq) and G(aq) are mixed together in a container. c A(aq) and F(aq) are mixed together in a container. d B(aq) and G(aq) are mixed together in a container. e Just B(aq) is placed into a container. f Just G(aq) is placed into a container. Consider any one of these situations in which a reaction does occur. At equilibrium, does the reaction mixture have appreciably more products than reactants? If not, how would you describe the equilibrium composition of the reaction mixture? How did you arrive at this answer?
Methanol, CH3OH, formerly known as wood alcohol, is manufactured commercially by the following reaction: CO(g)+2H2(g)CH3OH(g) A 1.500-L vessel was filled with 0.1500 mol CO and 0.3000 mol H2. When this mixture came to equilibrium at 500 K. the vessel contained 0.1187 mol CO. How many moles of each substance were in the vessel?
. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.
Antimony pentachloride decomposes according to this equation: SbCl5(g)SbCl3+Cl2(g) An equilibrium mixture in a 5.00-L flask at 443 C contains 3.85 g of SbCl5, 9.14 g of SbCl3, and 2.84 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?
Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C, only A, B, and C are present. The partial pressures of A, B, and D are given as PA, PB, and PD. Equilibrium is established 18 minutes after the reaction starts. Use terms is less than (LT), is greater than (GT), is equal to (EQ), or insufficient information (X) to answer the following questions. (a) PD at 5 min PA. (b) PA at 21 min PA at 27 min. (c) PB at 7 min PB at 13 min.(d) After 20 min, more B is added. When equilibrium is reestablished, K before the addition K after the addition. (e) After 20 min, the temperature is increased to 35C. PA before the temperature increase PA after the temperature increase after equilibrium is reestablished.
Suppose 1.000 mol CO and 3.000 mol H2 are put in a 10.00-L vessel at 1200 K. The equilibrium constant Kc for CO(g)+3H2(g)CH4(g)+H2O(g) equals 3.92. Find the equilibrium composition of the reaction mixture.
For the reactionN2O4(g)2NO2(g),Kp=0.25 at a certain temperature. If 0.040 atm of N2O4 is reacted initially, calculate the equilibrium partial pressures of NO2(g) and N2O4(g).
Solid ammonium iodide decomposes to ammonia and hydrogen gases at sufficiently high temperatures. NH4I(s)NH3(g)+HI(g)The equilibrium constant for the decomposition at 400C is 0.215. Twenty grams of ammonium iodide are sealed in a 7.50-L flask and heated to 400C. (a) What is the total pressure in the flask at equilibrium? (b) How much solid NH4I is left after the decomposition?

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