Sulfuryl chloride is used in
with Kc = 0.045 at 650 K.
- a A sample of 8.25 g of SO2Cl2 is placed in a 1.00-L reaction vessel and heated to 650 K. What are the equilibrium concentrations of all of the species?
- b What fraction of SO2Cl2 has decomposed?
- c If 5 g of chlorine is inserted into the reaction vessel, what qualitative effect would this have on the fraction of SO2Cl2 that has decomposed?
(a)
Interpretation:
The equilibrium composition of the given reaction mixture has to be found and the fraction of decomposition of
Concept introduction:
Equilibrium constant
Consider the reaction where the reactant A is giving product B.
On rearranging,
Where,
Answer to Problem 14.107QP
The equilibrium mixture contains
Explanation of Solution
Given,
The weight of
Molecular weight of
Volume of the vessel
Equilibrium constant
To find the initial concentration of
The concentration of
To find the equilibrium composition.
Using the table approach, the equilibrium concentrations of the reactants and the products can be found.
The equilibrium values are then substituted into the equilibrium expression to get the change in concentration x.
On rearranging we get a quadratic equation.
On solving the quadratic equation the value of x obtained.
On solving we get two values for x, the positive value for x is taken.
Hence,
(b)
Interpretation:
The equilibrium composition of the given reaction mixture has to be found and the fraction of decomposition of
Concept introduction:
Equilibrium constant
Consider the reaction where the reactant A is giving product B.
On rearranging,
Where,
Answer to Problem 14.107QP
The fraction of
Explanation of Solution
To find the fraction of
(c)
Interpretation:
The equilibrium composition of the given reaction mixture has to be found and the fraction of decomposition of
Concept introduction:
Equilibrium constant
Consider the reaction where the reactant A is giving product B.
On rearranging,
Where,
Answer to Problem 14.107QP
Addition of more amount of chlorine will shift equilibrium towards left and the rate of decomposition of
Explanation of Solution
According to Le Chatelier’s principle a system at equilibrium is disturbed, it will try to get the equilibrium state back by nullifying the disturbance. Addition of more product to the reaction mixture will shift the equilibrium towards left and the rate of decomposition decreases.
Want to see more full solutions like this?
Chapter 14 Solutions
General Chemistry - Standalone book (MindTap Course List)
- 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?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_forwardThe 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_forward
- At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?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
- At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forwardCyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5H9CH3) but with a different molecular structure. sssss The equilibrium constant has been estimated to be 0.12 at 25 C. If you had originally placed 0.045 mol of cyclohexane in a 2.8-L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established?arrow_forwardGaseous acetic acid molecules have a certain tendency to form dimers. (A dimer is a molecule formed by the association of two identical, simpler molecules.) The equilibrium constant Kc at 25C for this reaction is 3.2 104. a If the initial concentration of CH3COOH monomer (the simpler molecule) is 4.0 104 M, what are the concentrations of monomer and dimer when the system comes to equilibrium? (The simpler quadratic equation is obtained by assuming that all of the acid molecules have dimerized and then some of it dissociates to monomer.) b Why do acetic acid molecules dimerize? What type of structure would you draw for the dimer? c As the temperature increases would you expect the percentage of dimer to increase or decrease? Why?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author: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 LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning