Calcium oxide is used to remove the pollutant SO₂ from smokestack gases by the following exothermic reaction: 2 CaO (s) + 2 SO2 (g) + O2(g) CaSO4 (s) If the system was at equilibrium, what effect would each of the following have on the system. For your answer, indicate whether the reaction shifts to the left, shifts to the right, or no change to reestablish equilibrium. a. The concentration of SO₂ is decreased. b. Additional CaO is added to the system. c. The volume of the container the reaction is placed in decreases. d. The container that contains the reaction is heated in a hot water bath.

Calcium oxide is used to remove the pollutant SO₂ from smokestack gases by the following exothermic reaction: 2 CaO (s) + 2 SO2 (g) + O2(g) CaSO4 (s) If the system was at equilibrium, what effect would each of the following have on the system. For your answer, indicate whether the reaction shifts to the left, shifts to the right, or no change to reestablish equilibrium. a. The concentration of SO₂ is decreased. b. Additional CaO is added to the system. c. The volume of the container the reaction is placed in decreases. d. The container that contains the reaction is heated in a hot water bath.

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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