Questions: Given reaction: H2 + O2 -> H4O2 How much H4O2 can you make(in grams) if you had 20.3 g of H2 and unlimited amount of O2? A) 20.3 g B) 365 g C) 183 g D) 100 g

Solution Steps

The given reaction is: \[ \mathrm{H}_{2} + \mathrm{O}_{2} \rightarrow \mathrm{H}_{4} \mathrm{O}_{2} \]

However, this equation is not balanced. The correct balanced equation for the formation of hydrogen peroxide (\(\mathrm{H}_{2}\mathrm{O}_{2}\)) is: \[ 2\mathrm{H}_{2} + \mathrm{O}_{2} \rightarrow 2\mathrm{H}_{2}\mathrm{O}_{2} \]

• Molar mass of \(\mathrm{H}_{2}\) is \(2 \times 1.008 = 2.016 \, \text{g/mol}\).
• Molar mass of \(\mathrm{H}_{2}\mathrm{O}_{2}\) is \(2 \times 1.008 + 2 \times 16.00 = 34.016 \, \text{g/mol}\).

Given 20.3 g of \(\mathrm{H}_{2}\), calculate the moles of \(\mathrm{H}_{2}\): \[ \text{Moles of } \mathrm{H}_{2} = \frac{20.3 \, \text{g}}{2.016 \, \text{g/mol}} = 10.06 \, \text{mol} \]

From the balanced equation, 2 moles of \(\mathrm{H}_{2}\) produce 2 moles of \(\mathrm{H}_{2}\mathrm{O}_{2}\). Therefore, 10.06 moles of \(\mathrm{H}_{2}\) will produce 10.06 moles of \(\mathrm{H}_{2}\mathrm{O}_{2}\).

Convert moles of \(\mathrm{H}_{2}\mathrm{O}_{2}\) to grams: \[ \text{Mass of } \mathrm{H}_{2}\mathrm{O}_{2} = 10.06 \, \text{mol} \times 34.016 \, \text{g/mol} = 342.3 \, \text{g} \]

Final Answer