what amount of P4O10 was consumed? what mass of H3PO4 is produced?

Question

Use reaction stoichiometry to calculate amounts of reactants and products.

The substances perchloric acid (HClO4) and tetraphosphorus decaoxide react to form phosphoric acid and dichlorine heptaoxide.

Unbalanced equation: HClO4 (aq) + P4O10 (s) H3PO4 (aq) + Cl2O7 (l)

In one reaction, 68.8 g of Cl2O7 is produced. What amount (in mol) of P4O10 was consumed? What mass (in grams) of H3PO4 is produced?

_________ mol P4O10 consumed

_________g H3PO4 produced

Answer 1

12HClO₄ (aq) + P₄O₁₀ (s) ==> 4H₃PO₄ (aq) + 6Cl₂O₇ (l) ... balanced equation

molar mass Cl₂O₇ = 70.9 + 111.99 = 182.9 g/mol

moles Cl₂O₇ produced = 68.8 g x 1 mol/182.9 g = 0.376 moles

moles P₄O₁₀ consumed = 0.376 moles Cl₂O₇ x 1 mol P₄O₁₀/6 mol Cl₂O₇ = 0.0627 moles P₄O₁₀ consumed

mass H₃PO₄ produced = 0.376 mol Cl₂O₇ x 4 mol H₃PO₄/6 mol Cl₂O₇ x 98 g/mol = 24.6 g H₃PO₄

If there is something in this answer that you don't understand, please leave a comment