Question

How many moles of H3PO4 are produced when 71.0 g P4O10 reacts completely to form H3PO4?
P4O10(s) + H2O(l) → H3PO4(aq)

Answer 1

Answer:

1.00 mol

71.0g P4 0 10          1mol p4 0 10              4 moles H3 PO4

____________  x  ___________    x     ______________

      1                     283.886g P4 0 10           1mol P4 0 10

= 1.00 moles H3 PO4

Answer 2

1.00 moles of H₃PO₄ are produced

Given:

Mass of P₄O₁₀ = 71.0 g

To find:

Moles of H₃PO₄ = ?

Balanced chemical reaction:

P₄O₁₀(s) + H₂O(l) → H₃PO₄(aq)

Molar mass of P₄O₁₀ = 283.866 g or 284 g

Calculation for moles:

Number of moles is defined as given mass over molar mass.

$\text{Moles of } H_3PO_4= \frac{71.0 g P_4O_{10}}{1} \times \frac{1 mol P_4O_{10}}{283.886 g P_4O_{10}} \times \frac{4 moles H_3PO_4}{1 mol P_4O_{10}} \\\\\text{Moles of } H_3PO_4= 1.00 mol$

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