If 4.75 mL of cycohexene is reacted with 7.04 g of bromine, which is the limiting reagent? What is the theoretical yield of product?
Alkenes like cyclohexene undergo addition reactions with bromine to produce dibromoalkanes.
So, write and balance the equation.
Then, calculate how many moles of cyclohexene, and bromine you start with. Determine the limiting reageant from the coefficents and amount of moles given.
I will be happy to critique your thinking.
f 4.75 mL of cycohexene is reacted with 7.04 g of bromine, which is the limiting reagent? What is the theoretical yield of product?
To find the limiting reagent, we need to compare the number of moles of each reactant and see which one runs out first.
First, we need to write and balance the chemical equation:
Cyclohexene + Bromine -> Dibromoalkane
The stoichiometry of the reaction tells us that the ratio of cyclohexene to bromine is 1:1.
To determine the number of moles of cyclohexene, we need to know its molar mass. Let's assume it is 84 g/mol for this example.
moles of cyclohexene = (mass of cyclohexene in grams) / (molar mass of cyclohexene)
moles of cyclohexene = 4.75 mL (volume) * (density of cyclohexene in g/mL) / (molar mass of cyclohexene)
Similarly, for bromine:
moles of bromine = (mass of bromine in grams) / (molar mass of bromine)
Now that we have the moles of each reactant, we compare them in a 1:1 ratio to find the limiting reagent. Whichever reactant has fewer moles is the limiting reagent.
Finally, to calculate the theoretical yield of the product, we need to know the molar mass of the product and use the stoichiometry of the reaction.
theoretical yield = (moles of limiting reagent) * (molar mass of dibromoalkane) / (stoichiometric coefficient of limiting reagent)
Note that the theoretical yield assumes a 100% yield, which might not be realistic in all cases.
I hope this helps you understand how to determine the limiting reagent and calculate the theoretical yield!