Nitric oxide emitted from the engines of supersonic aircraft can contribute to the destruction of stratospheric ozone:
Nitric oxide emissions from supersonic aircraft can contribute to destruction ofthe ozone layer.
This reaction is highly exothermic
(a) Which rate constant is larger?
(b) The value of
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
EBK CHEMISTRY
- The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?arrow_forwardHydrogenation, the addition of hydrogen to an organic compound, is an industrially important reaction. Calculate rH, rS, and rG for the hydrogenation of octene, C8H16, to give octane, C8H19 at 25 C. Is the reaction product- or reactant-favored at equilibrium? C8H16(g) + H2(g) C8H18(g) Along with data in Appendix L, the following information is needed for this calculation.arrow_forwardHydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.arrow_forward
- Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?arrow_forwardSuppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forwardGiven these data at a certain temperature, 2H2(g)+O2(g)2H2O(g)Kc=3.21081N2(g)+3H2(g)2NH3(g)Kc=3.5108 calculate Kc for the reaction of ammonia with oxygen to give N2(g) and H2O(g).arrow_forward
- Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + 12 O2(g) SO3(g) K1 2SO3(g) 2SO2(g) + O2(g) K2 Which of the following expressions relates K1 to K2? (a) K2=K12 (b) K22=K1 (c) K2 = K1 (d) K2 = 1/K1 (e) K2=1/K12arrow_forward12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?arrow_forward. The reaction PCl3(l)+Cl2(g)PCl5(s)liberates 124 kJ of energy per mole of PCl3reacted. Will an increase in temperature shift the equilibrium position toward products or toward reactants?arrow_forward
- Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.arrow_forwardDuring an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?arrow_forwardPredict whether each of the following processes results in an increase in entropy in the system. (Define reactants and products as the system.) (a) Water vapor condenses to liquid water at 90 C and 1 atm pressure. (b) The exothermic reaction of Na(s) and Cl2(g) forms NaCl(s). (c) The endothermic reaction of H2 and I2 produces an equilibrium mixture of H2(g), I2(g), and HI(g). (d) Solid NaCl dissolves in water forming a saturated solution.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning