Question

A Review | Constants Periodic Table Correct Learning Goal: To calculate theoretical and percent yields, given the masses of multiple reactants. A balanced chemical reaction gives the mole ratios between reactants and products. For example, one mole of white phosphorus, P4, reacts with five moles of oxygen, O2, to produce two moles of diphosphorus pentoxide, P205: Part B What is the maximum number of moles of P2O5 that can theoretically be made from 144 g of O2 and excess phosphorus? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) P4 +502 +2P205 In this example, if we know the number of moles of phosphorus, we know that twice that much product can be made, assuming we have enough oxygen. Similarly, if we know the number of moles of oxygen, we know that two-fifths that much product can be made, assuming we have enough phosphorus. In a situation where you are given the mole amounts of both reactants, you should do this type of calculation individually for each one, finding two different values for the amount of product. The smaller of these two values is the maximum amount of product that can be made, also known as the theoretical yield. CHÅR O O ? Value Units Submit If you are given the masses of the reactants, you will first have to convert to moles. Once you have mole amounts, you can follow the procedure described above, applying the ratios shown in the balanced chemical equation. Part C Complete previous part(s) Part D Complete previous part(s)

Answer 1

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molar mass moles of a = mass of Oz - 1448m - u 1 molar mass 32gr/mole P4 +502 — 29,95 from 5 mol O2 -zma P2Os formed so 4.5 mole O₂ - 2x4.5 mol P₂O5 formed from mol of P2 Os formed 1-80 mol