If 3.00 moles of water are produced, how many moles of oxygen must be consumed?

I assume you are talking about the formation of water from its elements. If this is not true the following may need to be modified.
2H2 + O2 ==> 2H2O
3.00 mols H2O x (1 mol O2/2mol H2O) = ??

Didn't we just do this?

hji

10

To determine the number of moles of oxygen consumed, we need to use the balanced chemical equation for the reaction in which water is produced from oxygen.

The balanced chemical equation for the reaction of water formation from oxygen can be written as:

2 H2 + O2 -> 2 H2O

This equation tells us that for every 2 moles of H2 (hydrogen gas) consumed, 1 mole of O2 (oxygen gas) is also consumed, and 2 moles of H2O (water) are produced.

Now, we know that 3.00 moles of water are produced. Since the ratio of H2 to H2O is 2:2 (or 1:1), this means that 3.00 moles of water corresponds to 3.00 moles of H2 consumed.

To find the number of moles of oxygen consumed, we need to use the stoichiometric ratio from the balanced equation. Since the ratio of H2 to O2 is 2:1, we can set up a proportion:

(3.00 moles H2)/(2 moles O2) = X/(1 mole O2)

Simplifying the equation:

(3.00 moles H2) / (2) = X

X = (3.00 moles H2) / (2)

X = 1.50 moles O2

Therefore, 1.50 moles of oxygen must be consumed in the reaction to produce 3.00 moles of water.