Percent Yield Practice Problems

The reactants below combine according to the following equation: M₂ + 3 X₂ → 2 MX₃. The initial amounts of M₂ and X₂ are shown in Figure A (M = gray; X = orange) while the actual yield is shown in Figure B. What is the percent yield of the reaction?

The hydrogenation of pyridine (C₅H₅N) produces piperidine (C₅H₁₀NH). The actual yield of the reaction below is 83.0%. Calculate the mass of pyridine in grams produced from 42.5 g of pyridine (MW piperidine = 85.148 amu; MW pyridine = 79.1 amu).

The reaction of hydrochloric acid with manganese(IV) oxide produces chlorine as shown in the reaction below: 

4 HCl(aq) + MnO₂(s) → MnCl₂(aq) + 2 H₂O(l) + Cl₂(g) 

Consider the scenario where 95.50 g of MnO₂ is dissolved in a solution with 114.33 g of HCI

i. Identify the limiting reactant 

ii. Calculate the theoretical yield of Cl₂ in grams

iii. Calculate the actual yield of chlorine if the percent yield is 76.3 %

Consider the following reaction: 

2 Sb(s) + 3 S(s) → Sb₂S₃(s)

Calculate the percent yield of the reaction of 4.63 g of Sb(s) in excess S(s) if 2.31 g of Sb₂S₃ was actually produced. 

Consider the reaction for the recovery of metallic iron: 

Fe₂O₃ (s) + 3 H₂ (g) → 2 Fe (s) + 3 H₂O (g)

Calculate the percent yield of the reaction of 6.93 g of Fe₂O₃ in excess H₂ if 2.93 g of Fe (s) was actually produced. The molar mass of Fe₂O₃ is 159.7 g/mol. 

Consider the reaction below: 

2 NH₃ + OCl^- → N₂H₄ + Cl^- + H₂O

Calculate the moles of N₂H₄ as produced if 6.93 mol of NH₃ reacted and the reaction has a 85.6% yield

Consider the following reaction: 

4C₆H₅Cl + SiCl₄ + 8Na → (C₆H₅)₄Si + 8NaCl

 Calculate the mass of C₆H₅Cl will be required to make 163.2 g of (C₆H₅)₄Si if the reaction has a 91.1 % yield.