0.36 moles of each aluminum and oxygen react with each other to produce aluminum oxide. The amount of product formed is

Explanation

To determine the amount of product formed in a chemical reaction, we can use the stoichiometry of the reaction. The balanced chemical equation for the reaction between aluminum (Al) and oxygen (O₂) to produce aluminum oxide (Al₂O₃) is:4 Al + 3O2 ⇢ 2 Al2O3From the balanced equation, we can see that 4 moles of aluminum react with 3 moles of oxygen to produce 2 moles of aluminum oxide.Given that you have 0.36 moles of aluminum, we need to determine the limiting reactant. Since the stoichiometric ratio is 4:3 for aluminum to oxygen, we can find the moles of oxygen needed:Moles of O2 = (¾) * moles of AlMoles of O2= (¾) * 0.36Moles of O2= 0.27Now, we compare the moles of oxygen needed (0.27 moles) to the moles of oxygen provided (0.36 moles). Since we have more oxygen than needed, aluminum is the limiting reactant.The stoichiometry tells us that 4 moles of aluminum produce 2 moles of aluminum oxide. Therefore, 0.36 moles of aluminum will produce:Moles of Al2O3= (2/4) * moles of AlMoles of Al2O3= (2/4) * 0.36Moles of Al2O3= 0.18Therefore, the correct answer is (a) 0.18 mole, as this is the amount of aluminum oxide formed when 0.36 moles of aluminum react with the appropriate amount of oxygen.