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
Answer:
5.619 grams of diphosphorus pentoxide are formed when 2.45 g of phosphorus reacts with excess oxygen.
Explanation:
[tex]4P(s)+5O-2(g)\rightarrow 2P_2O_5(s)[/tex]
Mass of phosphorus = 2.45 g
Moles of phosphorous = [tex]\frac{2.45 g}{31 g/mol}=0.7903 mol[/tex]
According to reaction 4 moles of phosphorus gives 2 moles of diphosphorus pentoxide.
Then 0.7903 moles of phosphorus will give:
[tex]\frac{2}{4}\times 0.7903 mol=0.03957 mol[/tex] of diphosphorus pentoxide
Mass of 0.03957 moles of diphosphorus pentoxide :
[tex]0.03957 mol\times 142 = 5.619 g[/tex]
5.619 grams of diphosphorus pentoxide are formed when 2.45 g of phosphorus reacts with excess oxygen.
