Calculate the mass of Na₂O that can be produced by the reaction of 4.00 g of sodium and 2.00 g of oxygen in the reaction 4 Na + O₂ → 2 Na₂O.

Question

Quizplus · Accepted Answer

First, we need to determine which reactant limits the amount of product that can be formed. We can do this by calculating the moles of each reactant and comparing them. Moles of Na = 4.00 g / 23.00 g/mol = 0.174 mol Moles of O = 2.00 g / 16.00 g/mol = 0.125 mol Since O has the lower number of moles, it is the limiting reactant. This means that all of the O will be used up in the reaction and any extra Na will remain un-reacted. Now we can use stoichiometry to find the mass of the product that can be formed. From the balanced chemical equation, we know that 4 moles of Na reacts with 1 mole of O to form 2 moles of Na₂O. So, the number of moles of Na₂O formed can be calculated as: 0.125 mol O * (2 mol Na₂O / 1 mol O) = 0.25 mol Na₂O Finally, we can convert the number of moles to grams using the molar mass of Na₂O: Mass of Na₂O = 0.25 mol * 150.19 g/mol = 37.55 g However, we need to remember that we started with only 2.00 g of O. So, the actual amount of Na₂O that can be formed is limited by the amount of O, which means that it will be the smallest value we've calculated: Mass of Na₂O = 2.00 g * (0.25 mol / 0.125 mol) * (150.19 g/mol) = 5.39 g Therefore, the correct answer is D.

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Calculate the Mass of Na₂O That Can Be Produced by the Reaction