Sulfur dloxlde and oxygen react to form sulfur trioxide during one of the key steps In sulfuric acld synthesis. An industrial chemist studying this reaction fills a25.0 L tank with 2.0 mol of sulfur dioxide gas and 3.3 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxidegas to be 0.60 mol.Calculate the concentration equlibrlum constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2significant diglts.K = |CheckExplanationPrivacy Accessibili2021 McGraw-Hill Education. All Rights Reserved Terms of UseM9hpCeesc

SO2 reacts with O2 to form SO3 as per the equation 2SO2(g) + O2(g) <-----> 2SO3(g) Given ,…

Sulfur dioxlde and oxygen react to form sulfur trloxide during one of the key steps In sulfuric acld synthesis. An Industrial chemist studying this reaction fills a 25.0 L tank with 2.0 mol of sulfur dioxlde gas and 3.3 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trloxlde gas to be 0.60 mol. Calculate the concentration egulibrlum constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits.

Sulfur dioxlde and oxygen react to form sulfur trloxide during one of the key steps In sulfuric acld synthesis. An Industrial chemist studying this reaction fills a 25.0 L tank with 2.0 mol of sulfur dioxlde gas and 3.3 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trloxlde gas to be 0.60 mol. Calculate the concentration egulibrlum constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 44P

See similar textbooks

Similar questions

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.
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Draw a nanoscale (particulate) level diagram for an equilibrium mixture of
The density of trifluoroacetic acid vapor was determined at 118.1 C and 468.5 torr, and found to be 2.784 g/L. Calculate KC for the association of the acid.
Which of the systems described in Exercise 13.15 give homogeneous equilibria? Which give heterogeneous equilibria?
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
A small quantity of a soluble salt is placed in water. Equilibrium between dissolved and undissolved salt may or may not be attained. Explain.
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?
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)
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)
. 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?