# How many moles of water, H_2O, are produced from the reaction of 16 grams methane, CH_4. with an unlimited supply of oxygen, O_2?

## $C {H}_{4} + 2 {O}_{2} \to C {O}_{2} + 2 {H}_{2} O$

Are there not $\text{TWO moles}$ with respect to water?
$C {H}_{4} \left(g\right) + 2 {O}_{2} \left(g\right) \rightarrow C {O}_{2} \left(g\right) + 2 {H}_{2} O \left(l\right)$
And this tells you UNEQUIVOCALLY, that $16 \cdot g$ of methane gas reacts with $64 \cdot g$ of dioxygen gas to give $44 \cdot g$ of carbon dioxide gas, and $36 \cdot g$ of water. As always in a chemical reaction, MASS and charge are CONSERVED. What does this mean in the given context?