To find the moles of H₃PO₄ formed, let's first calculate the moles of P₄O₁₀ formed in the first reaction and then use that to calculate the moles of H₃PO₄ formed in the second reaction.
Step 1:Calculate moles of P₄O₁₀ formed in the first reaction.
Given that the yield of the first reaction is 70%, we can calculate the moles of P₄O₁₀ formed from 7 moles of P as follows:
Moles of P₄O₁₀ formed = 70% of 7 moles of P
[tex]Moles \: of \: P_4O_{10} \: formed = 0.70 \times 7 moles[/tex]
[tex]Moles \: of \: P_4O_{10} \: formed = 4.9 \: moles (approx.)[/tex]
Step 2:Calculate moles of H₃PO₄ formed in the second reaction.
In the second reaction, 1 mole of P₄O₁₀ reacts with H₂O to form 4 moles of H₃PO₄.
Given that the yield of the second reaction is 60%, we can calculate the moles of H₃PO₄ formed from the moles of P₄O₁₀ as follows:
Moles of H₃PO₄ formed = 60% of moles of P₄O₁₀ formed
Answers & Comments
Verified answer
Answer:
Approximately 2.94 moles of H₃PO₄ are formed.
Explanation:
To find the moles of H₃PO₄ formed, let's first calculate the moles of P₄O₁₀ formed in the first reaction and then use that to calculate the moles of H₃PO₄ formed in the second reaction.
Step 1: Calculate moles of P₄O₁₀ formed in the first reaction.
Given that the yield of the first reaction is 70%, we can calculate the moles of P₄O₁₀ formed from 7 moles of P as follows:
Moles of P₄O₁₀ formed = 70% of 7 moles of P
[tex]Moles \: of \: P_4O_{10} \: formed = 0.70 \times 7 moles[/tex]
[tex]Moles \: of \: P_4O_{10} \: formed = 4.9 \: moles (approx.)[/tex]
Step 2: Calculate moles of H₃PO₄ formed in the second reaction.
In the second reaction, 1 mole of P₄O₁₀ reacts with H₂O to form 4 moles of H₃PO₄.
Given that the yield of the second reaction is 60%, we can calculate the moles of H₃PO₄ formed from the moles of P₄O₁₀ as follows:
Moles of H₃PO₄ formed = 60% of moles of P₄O₁₀ formed
Moles of H₃PO₄ formed = 0.60 × 4.9 moles
Moles of H₃PO₄ formed = 2.94 moles (approx)
So, approximately 2.94 moles of H₃PO₄ are formed.
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