1. Write the balanced chemical equation:
The reaction of benzene with bromine (in the presence of a catalyst like FeBr3) is an electrophilic aromatic substitution reaction. The balanced equation is:
C₆H₆ + Br₂ → C₆H₅Br + HBr
2. Determine the limiting reactant:
* Calculate the moles of each reactant:
* Moles of benzene (C₆H₆) = (35.0 g) / (78.11 g/mol) = 0.448 mol
* Moles of bromine (Br₂) = (75.8 g) / (159.80 g/mol) = 0.474 mol
* Compare the mole ratio of reactants to the stoichiometric ratio: The balanced equation shows a 1:1 mole ratio between benzene and bromine. Since we have slightly more moles of bromine than benzene, benzene is the limiting reactant.
3. Calculate the theoretical yield of bromobenzene (C₆H₅Br):
* Use the mole ratio from the balanced equation: 1 mole of benzene produces 1 mole of bromobenzene.
* Convert moles of benzene to moles of bromobenzene:
* Moles of bromobenzene = 0.448 mol benzene
* Convert moles of bromobenzene to grams:
* Theoretical yield of bromobenzene = (0.448 mol) * (157.01 g/mol) = 70.4 g
Therefore, the theoretical yield of bromobenzene in this reaction is 70.4 grams.
