General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 13, Problem 13.112CHP
Consider the gas-phase decomposition of NOBr:
2 NOBr(g) ⇌ 2 NO(g) + Br2(s)
- (a) When 0.0200 mol of NOBr is added to an empty 1.00 L flask and the decomposition reaction is allowed to reach equilibrium at 300 K, the total pressure in the flask is 0.588 atm. What is the equilibrium constant Kc for this reaction at 300 K?
- (b) What is the value of Kp for this reaction at 300 K?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 13 Solutions
General Chemistry: Atoms First
Ch. 13.2 - The oxidation of sulfur dioxide to give sulfur...Ch. 13.2 - The following equilibrium concentrations were...Ch. 13.2 - Prob. 13.3PCh. 13.2 - The following pictures represent mixtures that...Ch. 13.3 - Prob. 13.5PCh. 13.4 - In the industrial synthesis of hydrogen, mixtures...Ch. 13.4 - Prob. 13.7PCh. 13.5 - Prob. 13.8PCh. 13.6 - Prob. 13.9PCh. 13.6 - Prob. 13.10P
Ch. 13.6 - Prob. 13.11CPCh. 13.6 - Prob. 13.12PCh. 13.6 - Prob. 13.13PCh. 13.6 - Prob. 13.14PCh. 13.6 - Prob. 13.15PCh. 13.6 - Prob. 13.16PCh. 13.8 - Prob. 13.17PCh. 13.9 - Prob. 13.18PCh. 13.9 - Prob. 13.19CPCh. 13.10 - Prob. 13.20PCh. 13.10 - Prob. 13.21PCh. 13.10 - Prob. 13.22CPCh. 13.11 - Prob. 13.23PCh. 13.11 - Prob. 13.24PCh. 13.11 - Prob. 13.25PCh. 13 - Consider the interconversion of A molecules (red...Ch. 13 - Prob. 13.27CPCh. 13 - Prob. 13.28CPCh. 13 - Prob. 13.29CPCh. 13 - Prob. 13.30CPCh. 13 - Prob. 13.31CPCh. 13 - Prob. 13.32CPCh. 13 - Prob. 13.33CPCh. 13 - Prob. 13.34CPCh. 13 - Prob. 13.35CPCh. 13 - Prob. 13.36CPCh. 13 - The following pictures represent the initial and...Ch. 13 - Prob. 13.38SPCh. 13 - Prob. 13.39SPCh. 13 - Prob. 13.40SPCh. 13 - Prob. 13.41SPCh. 13 - Prob. 13.42SPCh. 13 - Prob. 13.43SPCh. 13 - Prob. 13.44SPCh. 13 - Prob. 13.45SPCh. 13 - Prob. 13.46SPCh. 13 - Prob. 13.47SPCh. 13 - Prob. 13.48SPCh. 13 - Prob. 13.49SPCh. 13 - Prob. 13.50SPCh. 13 - Prob. 13.51SPCh. 13 - Prob. 13.52SPCh. 13 - Prob. 13.53SPCh. 13 - Prob. 13.54SPCh. 13 - Prob. 13.55SPCh. 13 - Prob. 13.56SPCh. 13 - Prob. 13.57SPCh. 13 - Prob. 13.58SPCh. 13 - Prob. 13.59SPCh. 13 - Prob. 13.60SPCh. 13 - Prob. 13.61SPCh. 13 - Prob. 13.62SPCh. 13 - Prob. 13.63SPCh. 13 - Prob. 13.64SPCh. 13 - Prob. 13.65SPCh. 13 - Prob. 13.66SPCh. 13 - Prob. 13.67SPCh. 13 - Prob. 13.68SPCh. 13 - Prob. 13.69SPCh. 13 - Prob. 13.70SPCh. 13 - Prob. 13.71SPCh. 13 - Prob. 13.72SPCh. 13 - Prob. 13.73SPCh. 13 - Gaseous indium dihydride is formed from the...Ch. 13 - Prob. 13.75SPCh. 13 - Prob. 13.76SPCh. 13 - Prob. 13.77SPCh. 13 - Prob. 13.78SPCh. 13 - Prob. 13.79SPCh. 13 - Prob. 13.80SPCh. 13 - Prob. 13.81SPCh. 13 - The value of Kc for the reaction of acetic acid...Ch. 13 - In a basic aqueous solution, chloromethane...Ch. 13 - Prob. 13.84SPCh. 13 - Prob. 13.85SPCh. 13 - Prob. 13.86SPCh. 13 - Prob. 13.87SPCh. 13 - Prob. 13.88SPCh. 13 - Prob. 13.89SPCh. 13 - Prob. 13.90SPCh. 13 - Prob. 13.91SPCh. 13 - Prob. 13.92SPCh. 13 - Consider the endothermic reaction Fe3+ (aq) + Cl...Ch. 13 - Prob. 13.94SPCh. 13 - Prob. 13.95SPCh. 13 - Prob. 13.96SPCh. 13 - Prob. 13.97SPCh. 13 - Prob. 13.98CHPCh. 13 - Prob. 13.99CHPCh. 13 - Prob. 13.100CHPCh. 13 - Prob. 13.101CHPCh. 13 - Prob. 13.102CHPCh. 13 - Prob. 13.103CHPCh. 13 - Prob. 13.104CHPCh. 13 - Prob. 13.105CHPCh. 13 - Refining petroleum involves cracking large...Ch. 13 - Prob. 13.107CHPCh. 13 - Prob. 13.108CHPCh. 13 - Prob. 13.109CHPCh. 13 - Prob. 13.110CHPCh. 13 - At 1000 K, Kp = 2.1 106 and H = 107.7 kJ for the...Ch. 13 - Consider the gas-phase decomposition of NOBr: 2...Ch. 13 - At 100C, Kc = 4.72 for the reaction 2 NO2(g) ...Ch. 13 - Prob. 13.114CHPCh. 13 - Prob. 13.115CHPCh. 13 - Prob. 13.116CHPCh. 13 - Prob. 13.117CHPCh. 13 - Prob. 13.118CHPCh. 13 - Prob. 13.119CHPCh. 13 - Prob. 13.120CHPCh. 13 - Prob. 13.121CHPCh. 13 - Prob. 13.122CHPCh. 13 - Prob. 13.123CHPCh. 13 - Prob. 13.124CHPCh. 13 - Prob. 13.125MPCh. 13 - Prob. 13.126MPCh. 13 - The equilibrium constant Kc for the gas-phase...Ch. 13 - Prob. 13.128MPCh. 13 - Prob. 13.129MPCh. 13 - Prob. 13.130MPCh. 13 - Prob. 13.131MPCh. 13 - Prob. 13.132MPCh. 13 - Consider the sublimation of mothballs at 27C in a...Ch. 13 - Prob. 13.134MPCh. 13 - Prob. 13.135MPCh. 13 - For the decomposition reaction PCl5(g) PCl3(g) +...Ch. 13 - Prob. 13.137MP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forwardAt a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?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_forward
- 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_forwardFor the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.arrow_forwardA solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.arrow_forward
- The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the initial concentration of PCl5 is 0.1000 M, what are the equilibrium concentrations of the reactants and products?arrow_forward12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.arrow_forwardFor the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?arrow_forward
- Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardKc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?arrow_forwardNitrosyl 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_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
General 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
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY