Limiting Reagent Practice Problems

Phenyl ethanoate is an odorant that can be found in passion fruit, black tea, and strawberries. It is produced synthetically from the reaction of phenol and ethanoic anhydride. 

(CH₃CO)₂O  (ethanoic anhydride) + C₆H₅OH (phenol) → CH₃COOC₆H₅ (phenyl ethanoate) + CH₃COOH (ethanoic acid)

Determine the theoretical yield of phenyl ethanoate if the reaction started with 63.0 g of phenol and 39.0 g of ethanoic anhydride.

The high-energy fuel 1,1-dimethylhydrazine reacts spontaneously with oxygen to give gaseous products according to the following reaction:

N₂H₂(CH₃)₂ (l) + O₂ (g) → CO₂ (g) + H₂O (g) + N₂ (g)    (unbalanced)

If 50.0 kg of this fuel is reacted with the same mass of oxygen, which of the two reactants will serve as the limiting reagent?

The organic compound 1,3-Dinitrobenzene is an explosive agent and a manufacturing by-product of TNT. Assuming that the nitration of nitrobenzene with the aid of a sulfuric acid catalyst and heat proceeds completely to give solely a 1,3-Dinitrobenzene product, identify the limiting reagent if 100 g of nitrobenzene and 100 g of nitric acid are reacted. 

C₆H₅NO₂ + HNO₃ → C₆H₄(NO₂)₂ + H₂O 

Dinitrobenzene is used in making dyes and explosives. Assume that the nitration of nitrobenzene with the aid of a sulfuric acid catalyst and heat proceeds completely to give solely a 1,3-Dinitrobenzene product. If the reaction started with 0.500 mol of nitrobenzene and 0.250 mol of nitric acid, calculate the theoretical yield (in g). 

C₆H₅NO₂ + HNO₃ → C₆H₄(NO₂)₂ + H₂O 

Shown below is a representation of a reaction mixture. A reaction proceeds according to the following balanced chemical equation: X₂ + 2 Y → 2 XY. Find the theoretical yield of the product. 

Consider 5.15 mol of aluminum metal is reacting 4.29 mol of oxygen. Calculate the aluminum oxide formed. 

Identify the limiting reagent if  212.5 g solid CaCO₃ is allowed to react with 160.0 g HCl and 46.8 grams of CO₂ is produced.

The balanced reaction is shown below: 

CaCO₃(s) + 2 HCl(aq) → CaCl₂(aq) + CO₂(g) + H₂O(l)

Calculate the moles of NO₂(g) required to react with 4.04 moles of H₂O to produce 10.76 moles of HNO₃

The balanced reaction is shown below:

3 NO₂ (g) + H₂O (l) → 2 HNO₃ (l) + NO (g)

Calculate the amount of excess reactant left after 11.3 mol ZnS and 18.3 mol O₂ react according to the following reaction: 

2 ZnS_(s) + 3 O_2(g)  → 2 ZnO_(s) + 2 SO_2(g)