H2 + CO2 <--> H2O + CO

if there were something that were added to this system to absorb the CO2, where would the equilibrium shift? Please don't just give the answer, explain as well, thanks :)

How about a little of neither. Le Chatelier's Principle, in not so eloquent terms, says that the reaction will shift so as to try and undo what we've done to it. So if we remove CO (not CO2) from the reaction it will shift to add more CO back. Which way is that? If you said right you would be right(correct).

Now if you remove CO2, it will try to add CO2 to replace what we've removed. Which way will it shift?

left?

yes

To determine how the equilibrium would shift when something is added to absorb CO2 from the given reaction, we need to understand Le Chatelier's principle. According to Le Chatelier's principle, when a system at equilibrium is subjected to a change in conditions (such as concentration, pressure, or temperature), the system will adjust in a way to partially counteract the change and restore equilibrium.

In this case, when something is added to absorb CO2, the concentration of CO2 will decrease. According to Le Chatelier's principle, the system will shift in the direction that counteracts the decrease in CO2 concentration. Therefore, the equilibrium will shift towards the reactant side (H2 + CO2).

This can be explained by considering the reaction's stoichiometry. When CO2 is removed, it affects the forward reaction (formation of products, H2O and CO) since CO2 is a reactant on the left side of the equation. To restore equilibrium, the system will try to replenish the lost CO2 by favoring the forward reaction. As a result, the equilibrium will shift towards the reactants in order to produce more CO2.

In summary, adding something to absorb CO2 will lower the concentration of CO2 and shift the equilibrium towards the reactant side (H2 + CO2).