Given the following equilibrium constants at 417°C,Naz0(s) + 2Na (1) + — О2(9) К, — 3 х 10 2-251NaO(g) = Na(1) +O2(9)2К, — 4х 10 5Naz O2 (s) = 2 Na(1) + O2 (9)NaO2 (s) = Na(1) + O2(g)K3 = 6 x 10-29K4 = 3 x 10-14determine the values for the equilibrium constants for the following reactions:1a. Naz 0(s) +02(9) = Na2O2(s)Equilibrium constantb. NaO(g) + Naz O(s) = NazO2(s) + Na(1)Equilibrium constant =c. 2 Na0(g) = Naz O2 (s)с.Equilibrium constant =(Hint: When reaction equations are added, the equilibrium expressions are multiplied.)

Answered: Image /qna-images/answer/33b596bc-4983-4016-8d57-751365c52b06.jpg

Given the following equilibrium constants at 417°C, Na20(s) = 2 Na(1) + 02 (9) K1 = 3 x 10-2 1 NaO(g) = Na(1) + O2(9) 2 K2 = 4 x 10-5 Naz O2 (s) = 2 Na(1) + O2 (9) NaO2 (s) = Na(1) + O2(g) K3 = 6 x 10-2 K4 = 3 x 10-14 determine the values for the equilibrium constants for the following reactions: 1 a. Naz 0(s) + O2(g) = NazO2 (s) Equilibrium constant = b. NaO(g) + Naz O(s) = NazO2(s) + Na(1) Equilibrium constant = c. 2 Na0(g) - Na2 O2 (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.)

Given the following equilibrium constants at 417°C, Na20(s) = 2 Na(1) + 02 (9) K1 = 3 x 10-2 1 NaO(g) = Na(1) + O2(9) 2 K2 = 4 x 10-5 Naz O2 (s) = 2 Na(1) + O2 (9) NaO2 (s) = Na(1) + O2(g) K3 = 6 x 10-2 K4 = 3 x 10-14 determine the values for the equilibrium constants for the following reactions: 1 a. Naz 0(s) + O2(g) = NazO2 (s) Equilibrium constant = b. NaO(g) + Naz O(s) = NazO2(s) + Na(1) Equilibrium constant = c. 2 Na0(g) - Na2 O2 (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...

See similar textbooks

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-.
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 product
At a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the equilibrium constant KP for the transformation at 60 C? H2O(l)H2O(g)
In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)
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?
Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.