Question

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of p4o10 (283.9 g/mol) with 12.00 g water (18.02 g/mol). What was the percent yield for this reaction? Include in your answer the balanced chemical equation.

Answer 1

The percent yield for the production of phosphoric acid from phosphorus(V) oxide and water is calculated using the actual yield and theoretical yield, with the balanced equation P4O10 + 6H2O → 4H3PO4. The answer to the student's question is a percent yield of 84.05%.

Step-by-step explanation:

The question asks about the percent yield for the reaction between phosphorus(V) oxide and water to form phosphoric acid. The balanced chemical equation for this reaction is:

P4O10 + 6H2O → 4H3PO4

To calculate the percent yield, you would first determine the limiting reagent, which in this case is phosphorus(V) oxide (P4O10). You would then calculate the theoretical yield of phosphoric acid formed using the molar mass of P4O10 and the amount used (10.00 g).

The actual yield of phosphoric acid is given as 11.60 g. To find the percent yield, use the formula:

Percent Yield = (Actual Yield/Theoretical Yield) x 100%

From the given information:

Moles of P4O10 = 10.00 g / 283.9 g/mol = 0.0352 mol

Since 1 mole of P4O10 produces 4 moles of H3PO4, the moles of H3PO4 produced would be 4 times 0.0352 mol = 0.1408 mol.

Theoretical Yield of H3PO4 = 0.1408 mol x 98.00 g/mol = 13.7984 g

Therefore:

Percent Yield = (11.60 g / 13.7984 g) x 100% = 84.05%