Consider the following equilibrium: AG = 41. KJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) about this system: 2NOCI (g) 2NO(g) + Cl₂ (g) Under these conditions, will the pressure of Cl, tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl, will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm x10 X at 878. °C. Answer the following questions

Consider the following equilibrium: AG = 41. KJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) about this system: 2NOCI (g) 2NO(g) + Cl₂ (g) Under these conditions, will the pressure of Cl, tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl, will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm x10 X at 878. °C. Answer the following questions

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat....

See similar textbooks

Similar questions

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?
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?
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.
In Section 17.3 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 for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
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?
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.
1. A process is spontaneous in the direction that moves it away from equilibrium toward equilibrium
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
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.
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.
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?