Reareproduced if the reaction begins with 3.0 grams of Al and 3.0 grams of FeO 2Al+3FeOarrow 1Al_(2)O_(3)+3Fe 1035 0.698 27.53 g 2335 Typoints

To determine the amount of product formed in the reaction, we need to follow these steps:1. Calculate the molar masses of the reactants and products.2. Convert the masses of the reactants to moles.3. Determine the limiting reactant.4. Calculate the amount of product formed.Given reaction: ### Step 1: Calculate Molar Masses- Molar mass of Al: - Molar mass of FeO: - Molar mass of Al₂O₃: - Molar mass of Fe: ### Step 2: Convert Masses to Moles- Moles of Al: - Moles of FeO: ### Step 3: Determine the Limiting ReactantFrom the balanced equation, the molar ratio of Al to FeO is 2:3.- Required moles of FeO for 0.111 moles of Al: Since we only have 0.042 moles of FeO, FeO is the limiting reactant.### Step 4: Calculate the Amount of Product FormedUsing the limiting reactant (FeO):- Moles of Al₂O₃ produced: - Mass of Al₂O₃ produced: Therefore, the amount of Al₂O₃ produced is .