M Wed Mar 15Consider the following chemical reaction at equilibrium:2NO₂(g) N₂O4(g)If the container's volume is increased by a factor of 2, while temperature is kept constant, howwill Keq for the reaction change?A) increaseQuestion 57 of 75B) decreaseC) stay the sameLTE 22%Subm 9 PM Wed Mar 15Consider the following chemical reaction at equilibrium:CO(g) + H₂O(g) = CO₂(g) + H₂(g)Question 58 of 75If H₂ is removed, in which direction will the equilibrium shift?A) reactantsB) productsC) neither the reactants nor the productsLTE 23%Submit

Given that, 1) 2NO2(g)<-------->N2O4(g) If volume of container increased by a factor of 2 at…

Consider the following chemical reaction at equilibrium: 2NO₂(g) N₂O4(g) If the container's volume is increased by a factor of 2, while temperature is kept constant, how will Keq for the reaction change? A) increase Question 57 of 75 B) decrease C) stay the same LIE 22% Submi

Consider the following chemical reaction at equilibrium: 2NO₂(g) N₂O4(g) If the container's volume is increased by a factor of 2, while temperature is kept constant, how will Keq for the reaction change? A) increase Question 57 of 75 B) decrease C) stay the same LIE 22% Submi

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 1ALQ: Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed...

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The following reaction occurs when a burner on a gas stove is lit: CH4+2O2(g)CO2(g)+2H2O(g) Is an equilibrium among CH4, O2, CO2, and H2O established under these conditions? Explain your answer.
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.
. Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?
. 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.
Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. (a) Write the expression for the equilibrium constant for the reversible reaction C(s)+H2O(g)CO(g)+H2(g)H=131.30kJ (b) What will happen to the concentration of each reactant and product at equilibrium if more C is added? (c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? (d) What will happen to the concentration of each reactant and product at equilibrium if CO is added? (e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?
. The reaction C2H2(g)+2Br2(g)C2H2Br4(g)is exothermic in the forward direction. Will an increase in temperature shift the position of the equilibrium toward reactants or products?
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 2NO(g)N2(g)+O2(g)K=11031 For each reaction, assume some quantities of the reactants were placed in separate containers and allowed to come to equilibrium. Describe the relative amounts of reactants and products that would be present at equilibrium. At equilibrium, which is faster, the forward or reverse reaction in each case?
A 1.604-g sample of methane (CH4) gas and 6.400 g oxygen gas are scaled into a 2.50-L vessel at 411C and are allowed to reach equilibrium. Methane can react with oxygen to form gaseous carbon dioxide and water vapor, or methane can react with oxygen to form gaseous carbon monoxide and water vapor. At equilibrium. the pressure of oxygen is 0.326 atm, and the pressure of water vapor is 4.45 atm. Calculate the pressures of carbon monoxide and carbon dioxide present at equilibrium.
Hydrogen for use in ammonia production is produced by the reaction CH4(g)+H2O(g)750oCNicatalystCO(g)+3H2(g) What will happen to a reaction mixture at equilibrium if a. H2O(g) is removed? b. the temperature is increased (the reaction is endothermic)? c. an inert gas is added to a rigid reaction container? d. CO(g) is removed? e. the volume of the container is tripled?
. Suppose are action has the equilibrium constant K=1.3108. 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?