The equilibrium expression for Keq for the reaction below is __________.2O3 ⇌ 3O2 (g)

Equilibrium is a state of a system in which reversible reaction takes place. Concentration of…

Answered: The equilibrium expression for Keq for…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.43PAE

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For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at 35.0C. If 2.00 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium?
Consider the following hypothetical dissociation: AB3(s) A3+(aq)+3 B(aq)H0What effect will each of the following have on the position of equilibrium? (a) addition of A(NO3)3 (b) increase in temperature (c) adding Na+, forming NaB
Write equilibrium expressions for each of the following equilibria. 2 C(s) + O2(g) «=* 2 CO(g) Zn (aq) + H2S(g) *=* ZnS(s) + 2 H (aq) HCl(g) + H2O(€) 5=i H,O+(aq) + Cl"(aq) (d) H2(g) + | O2(g) s=s H2O(g)
For the following endothermic reaction at equilibrium: 2SO3(g)2SO2(g)+O2(g) which of the following changes will increase the value of K? a. increasing the temperature b. decreasing the temperature c. removing SO3(g) (constant T) d. decreasing the volume (constant T) e. adding Ne(g) (constant T) f. adding SO2(g) (constant T) g. adding a catalyst (constant T)
A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
Write an equilibrium expression for each of the following gaseous reactions: a.3O22O3 b.COCl2CO+Cl2 c.CS2+4H2CH4+2H2S d.2SO2+O22SO3 e.CO+H2OCO2+H2
1. Which of the following is the correct form of the equilibrium constant expression for the decomposition of SO3 to SO2 and O2? Kc = [SO2][O2]/[SO3] Kc = [SO2]2[O2]/[SO3]2 Kc = [SO3]2/[SO2]2[O2] Kc = [SO2][O2]2
. Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
. Write the equilibrium expression for each of the following heterogeneous equilibria. a. 4Al(s)+3O2(g)2Al2O3(s)b. NH3(g)+HCl(g)NH4Cl(s)C. 2Mg(s)+O2(g)2MgO(s)
Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-81, for which of the diagrams is the numerical value of the equilibrium constant the smallest?
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?

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The equilibrium expression for Keq for the reaction below is __________. 2O3 ⇌ 3O2 (g)