Question- An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container.
CO(g) + H2O(g) <===> CO2(g) + H2(g)
How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol?
Anyone can tell me how to solve it step by step so that I will be able to understand what is going on?