$4Submit Answer000DOD F4The equilibrium constant, Kc, for the following reaction is 8.08 x 10-³ at 1080 K.2SO3 (9)2SO2(g) + O2(g)When a sufficiently large sample of SO3 (g) is introduced into an evacuated vessel at 1080 K, the equilibriumconcentration of O2 (g) is found to be 0.0980 M.Calculate the concentration of SO3 in the equilibrium mixture.[SO3] =MR%5Show HintATRetry Entire Group 9 more group attempts remainingViewing Your Aca...Have Changes in...F5[Review TopicsRavences]Use the References to access Important values if needed for this question.Cengage Learning Cengage Technical Support^6MacBook Air..F6Y&711F7U*8► 11F8Scholarship Ameri...(9F9O1bio 1108 chat0F10-P4)SAVAGE X FENTPrevious Next>F11+Save and Exit=F12

Answered: Image /qna-images/answer/760559a2-52b6-40e4-9e7b-9e4b95a767d8.jpg

the References to access Important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 8.08 x 10-3 at 1080 K. 2SO3(g)2SO2(g) + O2(g) When a sufficiently large sample of SO3 (g) Is Introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2 (g) is found to be 0.0980 M. Calculate the concentration of SO3 in the equilibrium mixture. [SO3] = M Submit Answer Retry Entire Group 9 more group attempts remaining

the References to access Important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 8.08 x 10-3 at 1080 K. 2SO3(g)2SO2(g) + O2(g) When a sufficiently large sample of SO3 (g) Is Introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2 (g) is found to be 0.0980 M. Calculate the concentration of SO3 in the equilibrium mixture. [SO3] = M Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 60QRT

See similar textbooks

Similar questions

Suppose 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?
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-.
At 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?
7-40 Is there any change in conditions that change the equilibrium constant, K, of a given reaction?
For 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?
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
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)
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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)
7-28 When the following reaction reached equilibrium at 325 K, the equilibrium constant was found to be 172. When a sample was taken of the equilibrium mixture, it was found to contain 0.0714 M NO2. What was the equilibrium concentration of N2O4?