Question

Phosphoric acid, H, PO, has some important applications. It can be used to produce fertilizers and it is present in soft drinks. Phosphoric acid can be made from phosphorus in a two step process: Reaction 1: P. +502 + P,00 Reaction 2: P,00 + 6H2O + 4H,PO 1. What is the molar mass of phosphoric acid, H3PO,? Report your answer to 3 significant figures. g/mol 2. How many moles of H, PO, can be produced from one mole of P, ? Hint: mol 3. A synthesis yielded 211 g of H3PO4. How many moles of H3PO, were produced? mol 4. How many moles of P would be required to produce the number of moles of H3PO, determined in question 3? mol 5. Convert the moles of P, determined in question 4 into grams. This will tell us the grams of P that actually reacted. Hint 6. Let's say that the experimentalist actually used 175 g from a bottle labeled Ps. Based on your answer to question 5, you can see that it did not all react. We will assume that this was because the reagent in this bottle contained inert impurities. Based upon your answer to question 5 and the mass of the reagent taken from the bottle labeled Ps, what was the actual mass percent of P4 in the bottle? Hint: ww

Answer 1

Reaction In Py +50₂ Puolo Reaction 2 PO + 6H₂O 4 H₂ Pou overall w Py+50₂ + 6H₂O - M₂ Poy. Y molar mans of hapoy = (1+3+31x1+ 16x4) Ilmal = 98.0g/mol 2 Ace to overall mole Py Hence, u mole & produce H₂Pou a mole produed H₂ Poy. from Imole of Py - mass of no. of ₂ poy mole of proclicced = 211g. H₂ Poy proclicced = man Molarmais = 2.153 mol 211g 98g med Pu. 4mal H₂ po prodhine by mal Py, then 2.153 mol H₂PO4 procure by 1 x 2,153 = 0.54 mol Mence, 0.54 mal Py required mass of Py = (0.54 x 124) = 66.96 g. Actuat viehet Actual Py = 66.96g reacted actual mass / Py in bottle = 66.96g. 175 g w/w Py in bottle = 38.26%