In the reaction of titanium and bromine, which would be the limiting reagent? I think it is bromine.
Ti + 2 Br2 = TiBr4
To determine the limiting reagent in a chemical reaction, you need to compare the mole ratio between the reactants and the balanced equation.
In the given reaction:
Ti + 2 Br2 = TiBr4
The mole ratio between titanium (Ti) and bromine (Br2) is 1:2. This means that for every one mole of titanium, two moles of bromine are required to fully react and form one mole of titanium tetrabromide (TiBr4).
To find the limiting reagent, you need to calculate the number of moles available for each reactant and compare them to the stoichiometric mole ratio.
Let's assume you have the following amounts of reactants:
- 3 moles of titanium (Ti)
- 4 moles of bromine (Br2)
To determine which reactant is the limiting reagent, follow these steps:
1. Calculate the moles of each reactant using their respective molar masses.
Molar mass of Ti = 47.87 g/mol
Molar mass of Br2 = 159.81 g/mol
Moles of Ti = Mass of Ti / Molar mass of Ti
= 3 mol
Moles of Br2 = Mass of Br2 / Molar mass of Br2
= 4 mol
2. Determine the stoichiometric ratio between the reactants.
From the balanced chemical equation, the stoichiometric ratio between Ti and Br2 is 1:2.
3. Calculate the moles of bromine required according to the stoichiometric ratio.
Moles of Br2 required = Moles of Ti × (2 moles of Br2 / 1 mole of Ti)
= 3 mol × (2 mol Br2 / 1 mol Ti)
= 6 mol Br2
4. Compare the moles of bromine required to the moles of bromine available.
In this case, 6 moles of bromine are required according to the stoichiometric ratio. However, you only have 4 moles of bromine available.
Since you have less bromine than is needed, bromine is the limiting reagent in this reaction.
Therefore, bromine will be completely consumed in the reaction, and some titanium will be left unreacted once all the bromine is used up.