For the following reaction, 6.56 grams of perchloric acid are mixed with excess tetraphosphorus decaoxide. The reaction yields 1.73 grams of phosphoric acid.

Question

For the following reaction, 6.56 grams of perchloric acid are mixed with excess tetraphosphorus decaoxide. The reaction yields 1.73 grams of phosphoric acid.

perchloric acid (aq) + tetraphosphorus decaoxide (s) ---> phosphoric acid (aq) + dichlorine heptaoxide (l)

What is the theoretical yield of phosphoric acid ? _____ grams

What is the percent yield of phosphoric acid ? ____%

Answer 1

Perchloric acid = HClO₄

Tetraphosphorous decaoxide = P₄O₁₀

Phosphoric acid = H₃PO₄

Dichlorine heptaoxide = Cl₂O₇

Write a correctly balanced equation:

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

Theoretical yield:

6.56 g HClO₄ x 1 mol HClO₄/100.46 g 4 moles H₃PO₄/12 moles HClO₄ x 97.99 g H₃PO₄/mol = 2.13 g H₃PO₄

Percent yield:

% yield = (actual yield/theoretical yield) x 100% = (1.73 g/2.13 g) x100% = 81.2% yield