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_10#? If 0.489 mol of phosphorus burns, what mass of oxygen is used? What mass of #P_4O_10# is produced?

#4P(s) + 5O_2(g) -> P_4O_10(s)#

1 Answer
Jul 7, 2017

Answer:

a. Grams P = 403 grams
b. Grams Oxy = 19.6 grams
c. Grams #P_4O_10# = 34.7 grams

Explanation:

Given #4P(s) + 5O_3(g) => P_4O_10(s)#

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

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

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