1 Consider the reaction:SO2(g) + 1/2 02(g)=s03(g)Write the equilibrium constant for this reaction in terms of the equilibrium constants, K1 and K2,for the reactions below:2 S(s) + 3 02(g)=2 S03(g) K1so2(g) K2S(s) + 02(g)For answers with both a subscript and a superscript, enter the subscript first. For example, enterK2 if the first equilibrium constant should be squared.K =

Answered: Image /qna-images/answer/7e90c873-cb3f-44fe-8499-bcc6a7ae4eec.jpg

Consider the reaction: SO2(g) + 1/2 02(g)=s03(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K1 and K2, for the reactions below: 2 S(s) + 3 02(g)=2 S03(g) K1 S(s) + 02(g) so2(g) K2 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K,2 if the first equilibrium constant should be squared. K =

Consider the reaction: SO2(g) + 1/2 02(g)=s03(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K1 and K2, for the reactions below: 2 S(s) + 3 02(g)=2 S03(g) K1 S(s) + 02(g) so2(g) K2 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K,2 if the first equilibrium constant should be squared. K =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 13QAP: Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant...

See similar textbooks

Similar questions

Consider the following hypothetical reactions and their equilibrium constants at 75C, 3A(g)3B(g)+2C(g)K1=0.31 3D(g)+2B(g)2C(g)K1=2.8 Find the equilibrium constant at 75C for the following reaction A(g)D(g)+53B(g)
The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
Distinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this say about a reaction? When Q K, what does this say about a reaction? When Q K. what does this say about a reaction?
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?
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Hydrogenation, 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.
Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.
Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?
What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5(l)C2H5OC2H5(g) at 25 C. {Vapor pressure was described in the previous Chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)
For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?
Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g) At a certain temperature, the equilibrium partial pressures of SO2, Cl2, and SO2Cl2 are 1.88 atm, 0.84 atm, and 0.27 atm, respectively. (a) What is K at that temperature? (b) Enough Cl2 condenses to reduce its partial pressure to 0.68 atm. What are the partial pressures of all gases when equilibrium is reestablished?