Question

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)`

Answer 1

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`