Consider the reaction: 2C0(g) + O2(g)=2CO2(g) AH° = -566 kJ Which of the following disturbances will shift the equilibrium to the right, forming more product? Link to Physical Constants Link to the Periodic Table a. Volume of the system is increased. O b. Partial pressure of CO2 is increased. O c. Partial pressure of O2 is increased. O d. Partial pressure of CO is increased. e. Temperature of the system is increased.

Consider the reaction: 2C0(g) + O2(g)=2CO2(g) AH° = -566 kJ Which of the following disturbances will shift the equilibrium to the right, forming more product? Link to Physical Constants Link to the Periodic Table a. Volume of the system is increased. O b. Partial pressure of CO2 is increased. O c. Partial pressure of O2 is increased. O d. Partial pressure of CO is increased. e. Temperature of the system is increased.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 66QAP: Consider the equilibrium H2(g)+S(s)H2S(g)When this system is at equilibrium at 25C in a 2.00-L...

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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.
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