EThe equilibrium constant, Kp, for the following reaction is 1.80 x 10-2 at 698 K.2HI(g) H₂(g) + 1₂ (9)80Submit AnswerIf an equilibrium mixture of the three gases in a 11.2 L container at 698 K contains HI at a pressure of 1.13 atm and H₂at a pressure of 1.03 atm, the equilibrium partial pressure of I2 isatm.$4000000RFF4VShow Hint%5Retry Entire Group 9 more group attempts remainingT[Review Topics][References]Use the References to access important values if needed for this question.GCengage Learning Cengage Technical SupportF5B6MacBook AirYH&7NF7J8FBIM-09KF9O<HOLDIO 1108 chatF10P4):;F11Previous{+ 11[altSAVAGE X FENTY...?#1Next>Save and ExitF121delete School Requirements: The Xeqreqnntent/takeCovalentActivity.do?locator assignment-takest to Withdr... Forms | Office of t... KB Viewing Your Aca... Have Changes in...ereg2req#2030 F3ECSubmit Answer$4000RFBlackboard Learn%The equilibrium constant, Kp, for the following reaction is 0.160 at 298 K.2NOBr(g) 2NO(g) + Br₂(g)If an equilibrium mixture of the three gases in a 17.8 L container at 298 K contains NOBr at a pressure of 0.301 atmand NO at a pressure of 0.376 atm, the equilibrium partial pressure of Br₂ isatm.Show Hint5TRetry Entire Group 9 more group attempts remainingFSCengage Learning Cengage Technical Support6X[Review Topics][References]Use the References to access important values if needed for this question.BMacBook AirYH&7NOWLV2 | Online teaching and XF7UJ0011FOIMScholarship Ameri...(9KF9O)OC Calculate the pOH of a 0.74Lbio 1108 chatF10BP4)AFIPrevious{+11=IÛSAVAGE X FENTY...?Next>XF1200+Tp #DSave and Exit2delete

1) we have to calculate the equilibrium partial pressure of I2 2) we have to calculate the…

The equilibrium constant, Kp, for the following reaction is 1.80 x 10-2 at 698 K. 2HI(g) H₂(g) + 1₂ (9) If an equilibrium mixture of the three gases in a 11.2 L container at 698 K contains HI at a pressure of 1.13 atm and H₂ at a pressure of 1.03 atm, the equilibrium partial pressure of I2 is atm.

The equilibrium constant, Kp, for the following reaction is 1.80 x 10-2 at 698 K. 2HI(g) H₂(g) + 1₂ (9) If an equilibrium mixture of the three gases in a 11.2 L container at 698 K contains HI at a pressure of 1.13 atm and H₂ at a pressure of 1.03 atm, the equilibrium partial pressure of I2 is atm.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter5: Introduction To Chemical Equilibrium

Section: Chapter Questions

Problem 5.16E: 5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of...

See similar textbooks

Similar questions

In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q were expressed in units of pressure. We also can use units of mol/L for the quantities in Q, specifical.ly for aqueous reactions. With this in mind, consider the reaction HF(aq)H+(aq)+F-(aq) for which Ka = 7.2 104 at 25C. Calculate G for the reaction under the following conditions at 25C. a. [HF] = [H+] = [F] = 1.0 M b. [HF] = 0.98 M, [H+] = [F] = 2.7 102M c. [HF] = [H+] = [F] = 1.0 105 M d. [HF] = [F] = 0.27 M, [H+] = 7.2 104M e. [HF] = 0.52 M, [F] = 0.67 M, [H+] = 1.0 103M Based on the calculated G values, in what direction will the reaction shift to reach equilibrium for each of the five sets of conditions?
. At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g)+O2(g)2NO(g)Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [N2]=0.041M. [O2]=0.0078M, and [NO]=4.710M. Calculate the value of K for the reaction.
Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, and arsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equation CaCO3(s)Ca2+(aq)+CO32(aq). Is Kc1,1, or 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation 3Ba2+(aq)+2PO43(aq)Ba3( PO4)2(s). Is Kc1,1, or 1? Explain your answer.
5.8. The hemoglobin in blood establishes an equilibrium with oxygen gas very quickly. The equilibrium can be represented as where “heme” stands for hemoglobin and “” stands for the hemoglobin-oxygen complex. The value for the equilibrium constant for this reaction is about . Carbon monoxide also binds with hemoglobin by the following reaction: This reaction has an equilibrium constant of . Which reaction’s equilibrium lies farther toward products? Does your answer justify the toxicity of ?
For the given chemical equilibrium, these data are determined experimentally: T K 350K 3.76102 450K 1.86101 Determine H for this reaction.
5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of sulfur that comes from combustion of S-containing materials, to , which can combine with to make sulfuric acid (and thus contribute to acid rain): (a) Write the expression for K for this equilibrium. (b) Calculate the value of for this equilibrium using the values in Appendix 2. (c) Calculate the value of K for this equilibrium. (d) If of and of are enclosed in a system in the presence of some liquid, in which direction would the reaction move?
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 system, K=4.86105 at 298K: HClO(aq)+F(aq)ClO(aq)+HF(aq) Assuming that you start with equal concentrations of HClO and F, and that no ClO or HF is initially present, which of the following best describes the equilibrium system: a the forward reaction is favored at equilibrium; b the reverse reaction is favored at equilibrium; c appreciable quantities of all species are present at equilibrium?
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)
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.
Hard water has a high concentration of calcium and magnesium ions. Focusing on the calcium ion, a common home water -softening process is based on a reversible chemical change that can be expressed by Na2Ze(s)+Ca2+(aq)CaZe(s)+2Na+(aq). Na2Ze represents a solid resin that is like an ionic compound between sodium ions and zeolite ions, a complex arrangement of silicate and aluminate groups; CaZe is the corresponding calcium compound. When, during the day, is this system most likely to reach equilibrium? Why doesnt it reach equilibrium and stay there? Periodically it is necessary to recharge the water softner by running salt water, NaCl(aq), through it. Why is this necessary? What concept is discussed in this chapter does the recharging process illustrate? Zeolite ions are used in home water softners because they have a porous but rigid structure that is weakly attracted to cations, readily allowing an exchange among different ions.
A student solved the following problem and found the equilibrium concentrations to be [SO2]=0.590M,[O2]=0.0450M, and [SO3]=0.260M. How could this student check the work without reworking the problem? The problem was: For the following reaction at 600 C: 2SO2(g)+O2(g)2SO3(g)Kc=4.32