Consider the reaction below, which is used in the industrial production of nickel (and which has already been featured in several problems this semester). You start with the reaction at equilibrium, with 4.0 atm of carbon monoxide and 3.0 atm of carbon dioxide. You add an unknown amount of CO. If, once equilibrium is reestablished, the amount of CO₂ is 4.0 atm, what pressure of CO did you add? NIO (s) + CO (g) Ni (s) + CO₂ (g)

Consider the reaction below, which is used in the industrial production of nickel (and which has already been featured in several problems this semester). You start with the reaction at equilibrium, with 4.0 atm of carbon monoxide and 3.0 atm of carbon dioxide. You add an unknown amount of CO. If, once equilibrium is reestablished, the amount of CO₂ is 4.0 atm, what pressure of CO did you add? NIO (s) + CO (g) Ni (s) + CO₂ (g)

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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Similar questions

A 4.72-g sample of methanol (CH3OH) was placed in an otherwise empty 1.00-L flask and heated to 250.C to vaporize the methanol. Over time, the methanol vapor decomposed by the following reaction: CH3OH(g)CO(g)+2H2(g) After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains 33.0 times as much H2(g) as CH3OH(g). Calculate K for this reaction at 250.C.
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.
A chemist wants to prepare phosgene, COCl2, by the following reaction: CO(g)+Cl2(g)COCl2(g) He places 4.00 g of chlorine, Cl2, and an equal molar amount of carbon monoxide, CO, into a 10.00-L reaction vessel at 395C. After the reaction comes to equilibrium, he adds another 4.00 g of chlorine to the vessel in order to push the reaction to the right to get more product. What is the partial pressure of phosgene when the reaction again comes to equilibrium? Kc = 1.23 103.
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?
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?
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.
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
. Equilibrium is microscopically dynamic but macroscopically static. Explain what this means.
Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br2(g)2Br(g) A 3.000-L flask initially contains pure molecular bromine. The temperature is then raised to 1600 K. If the total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm, what are the total moles of gas in the container? A spectroscopic analysis of this mixture showed that it contained 1.395 g of Br atoms. What is the partial pressure of Br? What is Kp for the dissociation of molecular bromine to bromine atoms?

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