Question

According to this equation, how much P4O10 can be produced from 8.32 g of phosphorus? 4 P + 5 O2 → P4O10

Answer 1

Answer:

38.28

Explanation:

4×8.32(p)=33.28         33.28+5=38.28

Answer 2

Considering the reaction stoichiometry, 19.05 grams of P₄O₁₀ can be produced from 8.32 g of phosphorus.

The balanced reaction is:

4 P + 5 O₂ → P₄O₁₀

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

• P: 4 moles
• O₂: 5 moles
• P₄O₁₀: 1 moles

The molar mass of each element or compound is:

• P: 31 g/mole
• O₂: 32 g/mole
• P₄O₁₀: 284 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

• P: 4 moles× 31 g/mole= 124 grams
• O₂: 5 moles× 32 g/mole= 160 grams
• P₄O₁₀: 1 moles× 284 g/mole= 284 grams

Then you can apply the following rule of three: if by stoichiometry 124 grams of P produces 284 grams of P₄O₁₀, 8.32 grams of P produces how much mass of P₄O₁₀?

$mass of P_{4} O_{10}=\frac{8.32 grams of Px284 grams of P_{4} O_{10}}{124 grams of P}$

mass of P₄O₁₀= 19.05 grams

Finally, 19.05 grams of P₄O₁₀ can be produced from 8.32 g of phosphorus.

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