For this reaction, the equilibrium constant, Keg, is 6.1 x 104 SO3 (g) O2 (g) + 2SO3 (g) Select the most accurate statement. O the equilibrium favors reactants O the rate of the forwards reaction is very fastfast O at equilibrium, the reaction mixture will contain a lot of both reactants and products the rate of the forwards reaction is very slow the equilibrium favors nroducts

For this reaction, the equilibrium constant, Keg, is 6.1 x 104 SO3 (g) O2 (g) + 2SO3 (g) Select the most accurate statement. O the equilibrium favors reactants O the rate of the forwards reaction is very fastfast O at equilibrium, the reaction mixture will contain a lot of both reactants and products the rate of the forwards reaction is very slow the equilibrium favors nroducts

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...

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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?
. For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular temperature. a. What does the very small equilibrium constant indicate about the extent to which oxygen gas, O2(g), is converted to ozone gas, O3(g), at this temperature? b. If the equilibrium mixture is analyzed and [O2(g)]is found to be 3.04102M, what is the concentration of O3(g) in the mixture’?
An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=* H+(aq) + COf-(aq) Assuming that the reactions in both directions are elementary' processes: Write rate expressions for the forward and reverse reactions. Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
. 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.
Consider the reaction N2O4(g)2NO2(g). Draw a graph illustrating the changes of concentrations of N2O4 and NO2 as equilibrium is approached. Describe how the rates of the forward and reverse reactions change as the mixture approaches dynamic equilibrium. Why is this called a dynamic equilibrium?
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When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
The equilibrium constant, Kc, is 1.05 at 350 K for the endothermic reaction 2 CH2Cl2(g) CH4(g) + CCl4(g) Which of the diagrams for Question 111 represents an equilibrium mixture at 350 K? Diagrams for Question 111.
12.103 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.
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?
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