I need help with a highschool chemistry question... Use the following reaction to solve the conversion problem 2 P2O4 = P4 + 5 O2

Question

a) how many grams of P4 could I produce from 71 grams of P2O5?
b) how many Liters of Oxygen gas could I produce from 213 grams of P2O5?
c) how many grams of P2O5 are required to produce 62 grams of P4?

Answer 1

2 P₂O₄  ==> P₄ + 5 O₂  is NOT a balanced equation because there are 8 oxygens on the left and 10 oxygens on the right. If the correct equation was meant to be 2 P₂O₄ ==> P₄ + 4 O₂ as a simple decomposition reactions, and I'm not certain this actually occurs, or if it was meant to be 2P₂O₄ + O₂ ==> P₄ + 5O₂, also not likely, then one could approach the solution. You should check the question again, and re-post.

EDITED: Just noticed it should be 2 P2O5 ==> P4 + 5O2 which is a balanced equation a) 71 g P2O5 x 1 mole/284 g = 0.25 moles P2O5 used 0.25 moles P2O5 x 1 mole P2/2 moles P2O5 = 0.125 moles P4 produced mass of P4 produced = 0.125 moles P4 x 123.9 g/mole = 15.5 g (3 significant figures) b) 213 g P2O5 x 1 mole/284 g = 0.75 moles P2O5 used 0.75 moles P2O5 x 5 moles O2/2 moles P2O5 = 1.875 moles O2 produced Volume O2 produced depends on temperature and pressure, but assuming it is STP, then... 1.875 moles O2 x 22.4 L/mole = 42 liters c) 62 g P4 x 1 mole P4/123.9 g = 0.500 moles P4 0.500 moles P4 x 2 moles P2O5/1 mole P4 = 1.00 moles P2O5 needed 1.00 moles P2O5 x 284 g/mole = 284 g P2O5 needed