Multiple Choice
In the reaction 2 H_2 + O_2 → 2 H_2O, how many grams of oxygen gas (O_2) are required to produce 36.0 grams of water (H_2O)?
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3. Chemical Reactions
Stoichiometry
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In the reaction 4Al + 3O_2 → 2Al_2O_3, what is the minimum number of grams of O_2 required to produce 1.00 mole of Al_2O_3?
A
24.0 g
B
16.0 g
C
32.0 g
D
48.0 g
Verified step by step guidance1
Identify the balanced chemical equation: \$4Al + 3O_2 \rightarrow 2Al_2O_3$.
Determine the mole ratio between \(O_2\) and \(Al_2O_3\) from the balanced equation. For every 2 moles of \(Al_2O_3\) produced, 3 moles of \(O_2\) are required.
Calculate the moles of \(O_2\) needed to produce 1.00 mole of \(Al_2O_3\) using the mole ratio: \(\text{moles of } O_2 = 1.00 \times \frac{3}{2}\).
Find the molar mass of \(O_2\). Since oxygen has an atomic mass of approximately 16.0 g/mol, the molar mass of \(O_2\) is \$2 \times 16.0$ g/mol.
Calculate the mass of \(O_2\) required by multiplying the moles of \(O_2\) by its molar mass: \(\text{mass of } O_2 = \text{moles of } O_2 \times \text{molar mass of } O_2\).
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