I am trying to find the theoretical yield and percent yield in nitrotoluene.
The question: Exactly 4.0 mL of toluene (density = 0.87 g/mL) were reacted with excess nitric acid in the presence of excess sulfuric acid, and 3.6 g of nitrotoluene were obtained.
So I started with the balanced equation: C7H8 + HNO3 --> C7H7NO2 + H2O
Then I calculated the grams of toluene: 4.0mL * 0.87g/mL = 3.48g C7H8
Then I calculated the moles of toluene: 3.48g * 1 mole/92.138g = 0.038 mole C7H8
Then I calculated the moles of nitrotoluene: 3.6g * 1 mole/137.136g = 0.026 mole C7H7NO2
This equation is a 1:1 ratio so I can't multiply by anything, so trying to find the limiting reactant is throwing me off especially since I don't know how much nitric acid is being used. Any suggestions on how to proceed?
