# 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?

## $4 P \left(s\right) + 5 {O}_{2} \left(g\right) \to {P}_{4} {O}_{10} \left(s\right)$

Jul 7, 2017

a. Grams P = 403 grams
b. Grams Oxy = 19.6 grams
c. Grams ${P}_{4} {O}_{10}$ = 34.7 grams

#### Explanation:

Given $4 P \left(s\right) + 5 {O}_{3} \left(g\right) \implies {P}_{4} {O}_{10} \left(s\right)$

a. $m a s s P = 4 \left(3.25 \text{moles")P = 13.00 "moles" P (31 g/"mole}\right) = 403 g$

b. $m a s s O = \frac{5}{4} \left(0.489 \text{mole") = 0.611 "mole"(32g/"mol}\right) = 19.6 g$

c. $m a s s {P}_{4} {O}_{10} = \frac{1}{5} \left(0.611 \text{mole")=0.122"mole"(284g/"mole}\right) = 34.7 g$