I am having such a hard time approaching this problem. It would be great if you can help me.

1.0 mole of CH4 react with 1.0 mole of O2 in a sealed container. (a) When the reaction is complete, what is the container? (b) How many moles of water are produced?
CH4 + 2O2 ---> CO2 + 2H2O

a) CH4 + O2 ---> CO2 + H2O

To determine the product when the reaction is complete, you need to follow the balanced chemical equation:

CH4 + 2O2 ---> CO2 + 2H2O.

(a) Looking at the equation, we can see that 1.0 mole of CH4 reacts with 1.0 mole of O2. So, for the reaction to be complete, all the reactants must be consumed. Therefore, the container after the reaction is complete will contain only the products CO2 and H2O.

(b) To find out how many moles of water are produced, you need to compare the stoichiometric ratio between CH4 and H2O in the balanced equation. The ratio is 1:2, meaning for every 1 mole of CH4, 2 moles of H2O are produced.

Since you have 1.0 mole of CH4, you can multiply this by the stoichiometric ratio to find the moles of water produced:

1.0 mole CH4 x (2 moles H2O / 1 mole CH4) = 2.0 moles H2O.

Therefore, 2.0 moles of water are produced when the reaction is complete.