Step 1: Reaction Overview
The chemical reaction: \[ 2H_2 + O_2 \rightarrow 2H_2O \] This shows 2 moles of hydrogen gas (\(H_2\)) react with 1 mole of oxygen gas (\(O_2\)) to make 2 moles of water (\(H_2O\)).
Step 2: Molar Masses
Molar mass of \(H_2\) = 2 g/mol
Molar mass of \(H_2O\) = 18 g/mol
Step 3: Water Production Calculation
With 10 g of \(H_2\), calculate moles of \(H_2\): \[ \text{Moles of } H_2 = \frac{10}{2} = 5 \text{ mol} \] From the balanced equation, 2 moles \(H_2\) yield 2 moles \(H_2O\). Thus, 5 moles \(H_2\) produce 5 moles \(H_2O\). Calculate water mass: \[ \text{Mass of } H_2O = 5 \text{ mol} \times 18 \text{ g/mol} = 90 \text{ g} \]
Step 4: Result
The water produced is 90 g. \[ \boxed{90 \text{ g of } H_2O} \]