Final answer:
The direction of the net reaction as new equilibrium is established varies depending on the external change. The removal of CO2 or increasing the volume favors the forward reaction; cooling favors the reverse reaction, while adding N2 or more graphite does not cause a shift.
Step-by-step explanation:
The direction of the net reaction as a new equilibrium is established can be predicted using Le Chatelier's principle. This principle states that if an external change is applied to a system at equilibrium, the system will adjust to partially offset the change and a new equilibrium will be established.
- a. CO2 is removed: The reaction will shift to the right (towards the products) to replace the removed CO2.
- b. Pressure is increased by adding N2(g): Since N2 is an inert gas and does not react with the system, the reaction will not shift in either direction.
- c. The vessel is cooled: Because the forward reaction is endothermic (consumes heat), cooling the system will shift the reaction to the left (towards the reactants) to absorb more heat.
- d. The volume is increased: Increasing the volume will decrease the pressure. Since we have more moles of gas on the product side, the reaction will shift to the right (towards the products) to increase pressure.
- e. More graphite is added: Adding more of the solid reactant graphite will not shift the equilibrium, as the concentration of solids does not affect the position of equilibrium in a reaction.