Phosphorus reacts with oxygen to form diphosphorus pentoxide, P2O5 . 4P(s)+5O2(g)⟶2P2O5(s) How many grams of P2O5 are formed whe n 2.45 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots
2 answers:
Answer:
5.619 grams of diphosphorus pentoxide are formed when 2.45 g of phosphorus reacts with excess oxygen.
Explanation:
Mass of phosphorus = 2.45 g
Moles of phosphorous =
According to reaction 4 moles of phosphorus gives 2 moles of diphosphorus pentoxide.
Then 0.7903 moles of phosphorus will give:
of diphosphorus pentoxide
Mass of 0.03957 moles of diphosphorus pentoxide :
5.619 grams of diphosphorus pentoxide are formed when 2.45 g of phosphorus reacts with excess oxygen.
Answer:
The answer to your question is:
Explanation:
2.45 g of Phosphorus
MW P = 31 g
MW P2O5 = 2(31) + 5(16) = 142 g
From the balance reaction
4 P ⇒ 2 P2O5
Then 4(31) g P ⇒ 2 (142) g P2O5
124g of P ⇒ 284 g of P2O5 Rule of three
2.45g P ⇒ x
x = 2.45 x 284/124 = 695.8/124 = 5.61 g of P2O5
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