Consider the following exothermic reaction, used to obtain lead from its ore: 2PbS (s) + 3O2 (g) + 2CO (g) ↔ 2 Pb (l) + 2SO2 (g) + 2CO2 (g) Assume that this reaction is in equilibrium. Given the following changes to the system, will the quantity of lead increase, decrease, or remain the same? iv) compressing the entire system. v) adding argon (an inert gas) vi) increasing the temperature
Consider the following exothermic reaction, used to obtain lead from its ore: 2PbS (s) + 3O2 (g) + 2CO (g) ↔ 2 Pb (l) + 2SO2 (g) + 2CO2 (g) Assume that this reaction is in equilibrium. Given the following changes to the system, will the quantity of lead increase, decrease, or remain the same? iv) compressing the entire system. v) adding argon (an inert gas) vi) increasing the temperature
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 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...
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Consider the following exothermic reaction, used to obtain lead from its ore:
2PbS (s) + 3O2 (g) + 2CO (g) ↔ 2 Pb (l) + 2SO2 (g) + 2CO2 (g)
Assume that this reaction is in equilibrium. Given the following changes to the system, will the quantity of lead increase, decrease, or remain the same?
iv) compressing the entire system.
v) adding argon (an inert gas)
vi) increasing the temperature
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