Answer:
\(359gO_{2}\)
Explanation:
1. Write the balanced equation:
\(_{2}H_{2}+O_{2}=_{2}H_{2}O\)
2. Find the quantity of \(H_{2}O\) produced by 45.2g of hydrogen:
\(45.2gH_{2}*\frac{1molH_{2}}{2.016gH_{2}}*\frac{2molesH_{2}O}{2molesH_{2}}*\frac{18gH_{2}O}{1molH_{2}O}= 404gH_{2}O\)
So, 45.2g of \(H_{2}\) produce 404g of \(H_{2}O\)
3. Find the quantity of \(O_{2}\) that reacted with 45.2g of \(H_{2}\):
\(404gH_{2}O*\frac{1molH_{2}O}{18gH_{2}O}*\frac{2molesO_{2}}{2molesH_{2}O}*\frac{16gO_{2}}{1molO_{2}}=359gO_{2}\)
