Answer:12 moles H2O
Explanation:
As you know, the stoichiometric coefficients attributed to each compound in the balanced chemical equation can be thought of as moles of reactants needed or moles of products formed in the reaction.
In your case, the balanced chemical equation for this synthesis reaction looks like this
2H2(g]+O2(g]→2H2O(l]]
Notice that the reaction requires 2 moles of hydrogen gas and 1 mole of oxygen gas to produce 2 moles of water.
This tells you that the reaction produces twice as many moles of water as you have moles of oxygen gas that take part in the reaction.
You know that your reaction uses 6.0 moles of oxygen. Assuming that hydrogen gas is not a limiting reagent, you can say that the reaction will produce
6.0moles O2⋅2 moles H2O1moles O2=12 moles H2O
