Need help Use the following information to answer numerical-response question 15.An Equilibrium SystemN₂(g) + C₂H₂(g) = 2 HCN(g)N₂(g) and C₂H₂(g) are injected into a closed 1.00 L flask and the system is allowed to reachequilibrium. The concentrations at equilibrium are recorded in the following data table.GasN₂(g)C₂H₂(g)HCN(g)EquilibriumConcentration (mol/L)0.4880.5130.0240Numerical Responsent15. The value of K, for the equilibrium system above, expressed in scientific notation, isa.bc x 10-d. The values of a, b, c, and d areandabсd(Record all four digits of your answer in the numerical-response section on the answer sheet.)bloow onesna

Given: N2(g)+C2H2(g)↔2HCN(g) Gas Equilibrium concentration (mol/L) N2 0.488 C2H2 0.513 HCN…

An Equilibrium System N₂(g) + C₂H₂(g) = 2 HCN(g) N₂(g) and C₂H₂(g) are injected into a closed 1.00 L flask and the system is allowed to reach equilibrium. The concentrations at equilibrium are recorded in the following data table. Numerical Response Gas N₂(g) C₂H₂(g) HCN(g) Equilibrium Concentration (mol/L) 0.488 0.513 0.0240 15. The value of K for the equilibrium system above, expressed in scientific notation, is a.bc x 10-d. The values of a, b, c, and d are. and b c a ." d (Record all four digits of your answer in the numerical-response section on the answer sheet.)

An Equilibrium System N₂(g) + C₂H₂(g) = 2 HCN(g) N₂(g) and C₂H₂(g) are injected into a closed 1.00 L flask and the system is allowed to reach equilibrium. The concentrations at equilibrium are recorded in the following data table. Numerical Response Gas N₂(g) C₂H₂(g) HCN(g) Equilibrium Concentration (mol/L) 0.488 0.513 0.0240 15. The value of K for the equilibrium system above, expressed in scientific notation, is a.bc x 10-d. The values of a, b, c, and d are. and b c a ." d (Record all four digits of your answer in the numerical-response section on the answer sheet.)

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 24A

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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?
The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.
Chemical Equilibrium II Magnesium hydroxide. Mg(OH)2, is a white, partially soluble solid that is used in many antacids. The chemical equation for the dissolving of Mg(OH)2(s) in water is Mg(OH)2(s)Mg2+(aq)+2OH(aq) a Describe a simple experimental procedure that you could use to study this solubility equilibrium. In your experiment, how would you determine when the solution process has attained equilibrium? b Write the equilibrium-constant expression for this dissolving of magnesium hydroxide. c Suppose equilibrium has been established in a container of magnesium hydroxide in water, and you decide to add more solid Mg(OH)2. What would you expect to observe? What effect will this addition of Mg(OH)2 have on the concentrations of Mg2+(aq) and OH(aq)? d Say you haw prepared an equilibrium solution of Mg(OH)2 by adding pure solid Mg(OH)2 to water. If you know the concentration of OH(aq), can you determine the concentration of Mg2+(aq)? If not, what information do you need that will allow you to determine the answer? e You slowly add OH from another source (say, NaOH) to an equilibrium mixture of Mg(OH)2 and water. How do you expect the concentration of the Mg2+(aq) to change? What might you be able to observe happening to the Mg(OH)2(s) as you add the OH? f Next you remove some, but not all, of the Mg(OH)2(s) from the mixture. How will this affect the concentrations of the Mg2+(aq) and OH(aq)? g If someone hands you a container of Mg(OH)2(aq) and there is no solid Mg(OH)2 present, is this solution at equilibrium? If it is not at equilibrium, what could you add to or remove from the container that would give an equilibrium system? h Consider an individual OH(aq) ion in an Mg(OH)2 solution at equilibrium. If you could follow this ion over a long period of time, would you expect it always to remain as an OH(aq) ion, or could it change in some way?