mochemetry and Equilibriur XO https://ezto.mheducation.com/hm.tpxConnectnochemistry and Equillbrlum (E Dempsey)Question 9 (of 10)Sec. Ex. 9- Equlibrium Decomposition of HIBe sure to answer all parts.The equilibrium constant K, for the reaction below is 81.3 at a certaintemperature.H2(g) + I2(g) S 2HI(g)If you start with 0.335 M hydrogen iodide, what will the concentrations of H2, I2, and HI be atequilibrium?[H2] =M[L2] =M[HI] =MReferencesO Type here to searchASUS V173.%24456. nochemistry and Equilibrur XÔ https://ezto.mheducation.com/hm.tpxQuestion 2 (of 10)Label the energy dlagrams and complete the statements about each.Label the energy diagrams below and complete the statements about each.EinitialreactantsproductsEfinalEinitialEfinalincreasesproductsreactantsEnnalEinitialdecreasesEgnalEntalEfinalEmitialstays thesamedecreasesincreasesΔΕAEdecreasesincreasesreleased toEnergy of systemEnergy of systemEnergy isreleased tosurroundings.Energy isabsorbedfromsurroundings.absorbedfromResetZoompe here to searchASUS VivoBookThis is it but this is wrong it doesn't saywhat's wrong tho19 home80DFKCValtS'Energy, EB.Energy, E

Be sure to answer all parts.The equilibrium constant K. for the reaction below is 81.3 at a certain temperature. H2(g) + I2(g) 5 2HI(g) If you start with 0.335 M hydrogen iodide, what will the concentrations of H2, I2, and HI be at equilibrium? [H2] = %3D [12] %3D M [HI] %3D

Be sure to answer all parts.The equilibrium constant K. for the reaction below is 81.3 at a certain temperature. H2(g) + I2(g) 5 2HI(g) If you start with 0.335 M hydrogen iodide, what will the concentrations of H2, I2, and HI be at equilibrium? [H2] = %3D [12] %3D M [HI] %3D

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 123CP: A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless,...

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The following reaction has KP=4.50105 at 720 K. N2(g)+3H2(g)2NH3 If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach equilibrium? P(NH3)=93atm,P(N2)=48atm, and P(H2)=52
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
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)
Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)
For which of the reactions in Exercise 13.15 does Kc (calculated using concentrations) equal KP (calculated using pressures)?
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?
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?
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
. 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 inter-conversion reaction?
For the given chemical equilibrium, these data are determined experimentally: T K 350K 3.76102 450K 1.86101 Determine H for this reaction.