At a certain temperature, nitrogen monoxide, NO(g), and hydrogen gas, H₂(g), are in a sealed container and are allowed to reach equilibrium. The equilibrium reaction is represented below. 2 NO(g) + 2 H₂(g) = N₂(g) + 2 H₂O(g) + 574.9 kJ Use the following information to answer questions 43 and 44 and numerical-response question 16. Row A. B. C. D. An Incomplete Equilibrium-law Expression [w] [x] [Y] [z]° 43. Which of the following rows identifies a location of the H₂(g) concentration in the incomplete equilibrium-law expression and the species favoured in the equilibrium reaction? Location of H₂(g) Concentration X X Z Z Kc = Species Favoured Kc = 0.05 Reactants Products Reactants Products

At a certain temperature, nitrogen monoxide, NO(g), and hydrogen gas, H₂(g), are in a sealed container and are allowed to reach equilibrium. The equilibrium reaction is represented below. 2 NO(g) + 2 H₂(g) = N₂(g) + 2 H₂O(g) + 574.9 kJ Use the following information to answer questions 43 and 44 and numerical-response question 16. Row A. B. C. D. An Incomplete Equilibrium-law Expression [w] [x] [Y] [z]° 43. Which of the following rows identifies a location of the H₂(g) concentration in the incomplete equilibrium-law expression and the species favoured in the equilibrium reaction? Location of H₂(g) Concentration X X Z Z Kc = Species Favoured Kc = 0.05 Reactants Products Reactants Products

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 99CP

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During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify 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.
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
. 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 the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the following changes affect the number of moles of each component of the system after equilibrium is re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst
. 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?
12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
. 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.
. For the reaction CO2(g)+H2(g)CO(g)+H2O(g)the equilibrium constant. K, has the value 5.21103at a particular temperature. If the system is analyzed at equilibrium at this temperature, it is found that [CO(g)]=4.73103M,[H2O(g)]=5.21103M, and [CO2(g)]=3.99102M. What is the equilibrium concentration of H2(g) in the system?
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