Answered: The equilibrium expression for Keq for…

Science

Chemistry

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

Chemistry for Today: General, Organic, and Biochemistry

9th Edition

ISBN:9781305960060

Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.40E

See similar textbooks

Similar questions

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)
The formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2 NH3(g) 1. Does the reaction shift to the right or to the left, or does it remain unchanged, when extra H2 is added? (a) shift left (b) shift right (c)unchanged
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?
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
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?
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?