Usng the following balanced chemical equation, determine the limiting reactant in the reaction between 3.0 grams of titanium and 8.0 grams of chlorine gas?
Ti(s) + 2Cl2(g) --> TiCl4(s)
ti= 3.0g/ 204.3833 =1.47 x 10^-2
cl2= 8.0/35.45 /2=1.1 x 10^-1
ti is the Lr since it produces less product.
Moles of Ti = 3.0g / 47.87g/mol = 0.0627 moles Ti
8.0g Cl2 / 70.9g/mol = 0.113 mol Cl2
Available ratio:
(0.113 mol Cl2) / (0.0627 moles Ti) =
1.80 mol Cl2 / 1mole Ti
Needed Ratio:
The Cl2 / Ti mole ratio in the balanced chemical equation =
2 mol Cl2 / 1 mol Ti
The comparison of the mole ratio in the mixture to the mole ratio needed shows we don't have enough Cl2 to react with all the Ti metal. So, Cl2 is the Limiting Reagent, and Ti is used in excess.
To determine the limiting reactant, we need to compare the amount of each reactant to the stoichiometry of the balanced chemical equation. The reactant that produces the least amount of product (TiCl4 in this case) is the limiting reactant.
To find the limiting reactant, follow these steps:
Step 1: Convert the mass of each reactant to moles.
- Titanium (Ti):
Molar mass of Ti = 47.87 g/mol
Moles of Ti = Mass of Ti / Molar mass of Ti
= 3.0 g / 47.87 g/mol
- Chlorine gas (Cl2):
Molar mass of Cl2 = 2 * 35.45 g/mol = 70.90 g/mol
Moles of Cl2 = Mass of Cl2 / Molar mass of Cl2
= 8.0 g / 70.90 g/mol
Step 2: Use the stoichiometric ratio from the balanced equation to determine the moles of product that can be formed from each reactant.
From the balanced equation:
1 mole of Ti reacts with 2 moles of Cl2 to produce 1 mole of TiCl4.
Moles of TiCl4 produced from Ti = Moles of Ti * (1 mole of TiCl4 / 1 mole of Ti)
Moles of TiCl4 produced from Cl2 = Moles of Cl2 * (1 mole of TiCl4 / 2 moles of Cl2)
Step 3: Compare the moles of TiCl4 produced from each reactant.
The reactant that produces the smallest number of moles of TiCl4 is the limiting reactant.
Step 4: Convert the moles of the limiting reactant back to grams of the limiting reactant, if needed.
Now you have the information required to determine the limiting reactant in the given reaction. Follow the steps above while using the given masses of titanium and chlorine gas to complete the calculations and find the limiting reactant.