If 10 mols of Hydrogen gas was available to react with excess Oxygen, how many grams of water would be produced? 2H_(2)+O_(2)otimes 2H_(2)O 180 g 90.0 g 3.6 g 45.0 g

## Step1: Determine the Molar Mass of Water<br />### Calculate the molar mass of water ($H_2O$) by adding the atomic masses of its constituent elements: $2 \times 1.01 \, \text{g/mol}$ for hydrogen and $16.00 \, \text{g/mol}$ for oxygen, resulting in $18.02 \, \text{g/mol}$.<br />## Step2: Use Stoichiometry to Find Moles of Water Produced<br />### According to the balanced chemical equation $2H_{2} + O_{2} \rightarrow 2H_{2}O$, 2 moles of $H_2$ produce 2 moles of $H_2O$. Therefore, 10 moles of $H_2$ will produce 10 moles of $H_2O$.<br />## Step3: Convert Moles of Water to Grams<br />### Multiply the moles of water (10 moles) by the molar mass of water (18.02 g/mol) to find the mass of water produced: $10 \times 18.02 = 180.2 \, \text{g}$.