Phosphorus burns in air to produce a phosphorus oxide in the following reaction. What mass of phosphorus will be needed to produce 3.25 mol of P_4O_10P4O10? If 0.489 mol of phosphorus burns, what mass of oxygen is used? What mass of P_4O_10P4O10 is produced?

4P(s) + 5O_2(g) -> P_4O_10(s)4P(s)+5O2(g)→P4O10(s)

1 Answer
Doc048
Jul 7, 2017

a. Grams P = 403 grams
b. Grams Oxy = 19.6 grams
c. Grams P_4O_10P4O10 = 34.7 grams

Explanation:

Given 4P(s) + 5O_3(g) => P_4O_10(s)4P(s)+5O3(g)⇒P4O10(s)

a. mass P = 4(3.25 "moles")P = 13.00 "moles" P (31 g/"mole") = 403gmassP=4(3.25moles)P=13.00molesP(31gmole)=403g

b. mass O = 5/4(0.489 "mole") = 0.611 "mole"(32g/"mol") = 19.6 gmassO=54(0.489mole)=0.611mole(32gmol)=19.6g

c. mass P_4O_10 = 1/5(0.611"mole")=0.122"mole"(284g/"mole")=34.7gmassP4O10=15(0.611mole)=0.122mole(284gmole)=34.7g

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