To determine the maximum amount of aluminum oxide (Al₂O₃) that can be produced from the reaction of aluminum (Al) and oxygen (O₂), we first need to understand the balanced chemical equation for the reaction. ### Step 1: Write the Balanced Chemical Equation The reaction between aluminum and oxygen can be represented by the following balanced equation: \[ 4 \text{Al} + 3 \text{O}_2 \rightarrow 2 \text{Al}_2\text{O}_3 \] This equation tells us that 4 moles of aluminum react with 3 moles of oxygen to produce 2 moles of aluminum oxide. ### Step 2: Analyze the Stoichiometry From the balanced equation, we can see the stoichiometric relationships: - 4 moles of Al produce 2 moles of Al₂O₃. - Therefore, for every 4 moles of aluminum, we get 2 moles of aluminum oxide. ### Step 3: Calculate the Maximum Amount of Aluminum Oxide To find out how much aluminum oxide can be produced from 4 moles of aluminum, we can set up a proportion based on the stoichiometry of the reaction: \[ \text{If } 4 \text{ moles of Al} \rightarrow 2 \text{ moles of Al}_2\text{O}_3 \] We can calculate the amount of Al₂O₃ produced from 4 moles of Al: \[ \text{Moles of Al}_2\text{O}_3 = \left( \frac{2 \text{ moles Al}_2\text{O}_3}{4 \text{ moles Al}} \right) \times 4 \text{ moles Al} = 2 \text{ moles Al}_2\text{O}_3 \] However, we need to consider the total amount of Al₂O₃ produced based on the complete reaction of both reactants. ### Step 4: Consider the Oxygen The balanced equation also indicates that 3 moles of O₂ are required for the reaction. Since we have 4 moles of Al, we need to check if we have enough O₂ to react with it. Using the stoichiometry again: \[ \text{If } 3 \text{ moles of O}_2 \rightarrow 2 \text{ moles of Al}_2\text{O}_3 \] We can calculate how much Al₂O₃ can be produced from 3 moles of O₂: \[ \text{Moles of Al}_2\text{O}_3 = \left( \frac{2 \text{ moles Al}_2\text{O}_3}{3 \text{ moles O}_2} \right) \times 3 \text{ moles O}_2 = 2 \text{ moles Al}_2\text{O}_3 \] ### Step 5: Conclusion Since both reactants (Al and O₂) produce the same amount of Al₂O₃ (2 moles), we can conclude that the maximum amount of aluminum oxide produced is 2 moles. However, the question states that we are assuming complete reaction and no limiting reactants, which means we are looking for the theoretical yield based on the stoichiometry of the reaction. ### Final Answer The maximum amount of aluminum oxide that can be produced is **2 moles** of Al₂O₃. ### Explanation of Other Options - **Option A (2 moles)**: This is the correct answer based on the stoichiometry of the reaction. - **Option B (4 moles)**: This option is incorrect because it suggests that 4 moles of Al would produce 4 moles of Al₂O₃, which is not supported by the balanced equation. - **Option C (6 moles)**: This option is incorrect as it implies that more Al₂O₃ can be produced than the stoichiometry allows. - **Option D (8 moles)**: This option is incorrect because it suggests that the reaction can produce 8 moles of Al₂O₃, which is not possible given the amounts of reactants. ### Revision Summary - The balanced equation for the reaction is \(4 \text{Al} + 3 \text{O}_2 \rightarrow 2 \text{Al}_2\text{O}_3\). - 4 moles of Al produce 2 moles of Al₂O₃. - 3 moles of O₂ also produce 2 moles of Al₂O₃. - The maximum amount of aluminum oxide produced is 2 moles, confirming that option A is correct.