How many grams of water could be made from 5.0 mol H_2 and 3.0 mol O_2?

Mar 27, 2017

You need a stoichiometric equation to represent the formation of water:

Explanation:

${H}_{2} \left(g\right) + \frac{1}{2} {O}_{2} \left(g\right) \rightarrow {H}_{2} O \left(l\right)$

Given the stoichiometry, dihydrogen is in deficiency, and ONLY $2.5 \cdot m o l$ dioxygen will react to give $5 \cdot m o l$ water.

And this represents a mass of $5 \cdot \cancel{m o l} \times 18.01 \cdot g \cdot \cancel{m o {l}^{-} 1} = 90 \cdot g$.

What mas of dioxygen will remain after reaction?

Mar 27, 2017

The balanced equation is: $2 {H}_{2} \left(g\right) + {O}_{2} \left(g\right) \to 2 {H}_{2} O \left(l\right)$