Chemistry question: how will a system having the following equilibrium in it respond to these changes

CO2(g) + H2O(g) <-----> H2(g) + CO2 + heat

a. Removing CO?
b. Adding water vapor?
c. Increasing system temperature?

How will a system having the following equilibrium in it respond to each of those changes listed above? Please help :D

You have a typo here.
CO2(g) + H2O(g) <-----> H2(g) + CO2 + heat

The reaction is between carbon monoxide and water vapor to make carbon dioxide and hydrogen gas:
CO(g) + H2O(g) <==> H2(g) + CO2(g) + heat

According to Le Chatelier's principle, removing CO(g) will cause a shift in the equilibrium to the left in order to make more CO. It will reduce the partial pressures of H2 and CO2

According to Le Chatelier's principle, adding H2O(g) will cause a shift in the equilibrium to the right in order to reduce the partial pressure of water vapor. It will make more H2 and CO2.

Increasing the temperature is the equivalent of adding heat, and according to Le Chatelier's principle, adding heat will shift the equilibrium to the left to reduce the amount of added heat. It will make more CO2 and H2O and reduce the partial pressures of H2 and CO2.

CO(g) + H2O(g) <-----> H2(g) + CO2 + heat
a shift left
b shift right
c shift left