We’re being asked to calculate the mass of Al2O3, which will be formed by 4.6 g Al with excess O2. Since O2 is in excess, we can simply ignore it in our calculations. The flow for this problem will be like this:
Mass of Al (molar mass of Al) → Moles of Al (mole-to-mole comparison) → Moles of Al2O3 (molar mass of Al2O3) → Mass of Al2O3
Aluminum and oxygen react according to the following equation: 4Al(s) + 3O 2(g) → 2Al2O3(s)
What mass of Al2O3, in grams, can be made by reacting 4.6 g Al with excess oxygen?
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Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry. Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems.
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Our tutors rated the difficulty ofAluminum and oxygen react according to the following equatio...as low difficulty.
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Based on our data, we think this problem is relevant for Professor O'Connor's class at CSU OHIO.