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?

Question

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

Owen Ambrose · Accepted Answer

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

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#

Cooper Adams · Answer

undefined To determine the mass of phosphorus needed to produce 3.25 mol of P4O10, we use the stoichiometry of the reaction:

4P + 5O2 -> P4O10

From the balanced equation, 1 mol of P4O10 requires 4 mol of phosphorus. Therefore, to produce 3.25 mol of P4O10, we need:

3.25 mol P4O10 * (4 mol P / 1 mol P4O10) = 13 mol P

Now, to find the mass of phosphorus needed:

13 mol P * (30.97 g/mol P) = 402.61 g P

For the second part, if 0.489 mol of phosphorus burns, we use the stoichiometry to find the amount of oxygen used:

0.489 mol P * (5 mol O2 / 4 mol P) = 0.61125 mol O2

To find the mass of oxygen used:

0.61125 mol O2 * (32 g/mol O2) = 19.56 g O2

Lastly, to find the mass of P4O10 produced:

0.489 mol P * (1 mol P4O10 / 4 mol P) * (284.9 g/mol P4O10) = 35.75 g P4O10