Consider the unbalanced reaction Ti(s) + Cl2(g) --> TiCl4(s)
When 10.3 g of Ti react with 12.7 g of Cl2, 16.2 g of TiCl4 are obtained. The theoretical yield of TiCl4 is
, the limiting reactant is
and the percent yield is
%. (Remember to use correct sig figs)
To find the theoretical yield of TiCl4, we need to determine which reactant is the limiting reactant. The limiting reactant is the reactant that is completely consumed in the reaction, thus determining how much product can be formed.
Let's calculate the number of moles of each reactant using their molar masses:
Molar mass of Ti = 47.867 g/mol
Number of moles of Ti = (mass of Ti / molar mass of Ti) = (10.3 g / 47.867 g/mol) ≈ 0.215 mol
Molar mass of Cl2 = 70.906 g/mol
Number of moles of Cl2 = (mass of Cl2 / molar mass of Cl2) = (12.7 g / 70.906 g/mol) ≈ 0.179 mol
Next, we need to calculate the stoichiometric ratio of Ti and TiCl4 in the balanced equation:
From the balanced equation: 1 mole of Ti reacts with 1 mole of TiCl4
Based on the stoichiometric ratio, the amount of TiCl4 that would be formed from 0.215 mol of Ti is also 0.215 mol.
To find the theoretical yield of TiCl4 in grams, we multiply the number of moles by the molar mass of TiCl4:
Molar mass of TiCl4 = 189.692 g/mol
Theoretical yield of TiCl4 = (number of moles of TiCl4 × molar mass of TiCl4)
Theoretical yield of TiCl4 = (0.215 mol × 189.692 g/mol) ≈ 40.833 g
Therefore, the theoretical yield of TiCl4 is approximately 40.833 g.
To determine the limiting reactant, we compare the number of moles used with the stoichiometric ratio of the balanced equation. We can see that for Ti, we have 0.215 mol available, but for Cl2, we have only 0.179 mol. Since Cl2 is less than Ti, Cl2 is the limiting reactant.
Finally, let's calculate the percent yield of TiCl4:
Percent yield = (actual yield / theoretical yield) × 100
Given: actual yield = 16.2 g (from the question)
Percent yield = (16.2 g / 40.833 g) × 100 ≈ 39.6%
Therefore, the percent yield of TiCl4 is approximately 39.6%.
Balanced equation: Ti + 2Cl2 --> TiCl4
To find the limiting reactant find the moles of Ti and Cl2. Remeber that theres 2 moles of Cl2. The one with the lowest amount of moles is the limiting reactant.
Next use the moles of the limiting reagent to find to theoretical mass yield. You do this by converting the limiting reactants moles to the moles of TiCl4 and then multiply by the molecular mass of TiCl4 to find the theoretical mass.
% Yield= (Theoretical mass/16.2) *100
Sorry the % yield is = (16.2/ theoretical yield) *100
To determine the theoretical yield, limiting reactant, and percent yield, we need to follow a few steps.
Step 1: Write and balance the chemical equation.
The balanced equation for the reaction is:
Ti(s) + 2Cl2(g) --> TiCl4(s)
Step 2: Calculate the molar masses.
The molar mass of Ti is 47.87 g/mol.
The molar mass of Cl2 is 35.45 g/mol.
Step 3: Convert the given masses to moles.
Given:
Mass of Ti = 10.3 g
Mass of Cl2 = 12.7 g
Moles of Ti = (Mass of Ti) / (Molar mass of Ti)
Moles of Ti = 10.3 g / 47.87 g/mol
Moles of Cl2 = (Mass of Cl2) / (Molar mass of Cl2)
Moles of Cl2 = 12.7 g / 35.45 g/mol
Step 4: Determine the stoichiometry.
From the balanced equation, it can be seen that 1 mole of Ti reacts with 2 moles of Cl2 to produce 1 mole of TiCl4.
So, the moles of Cl2 required for the reaction can be calculated as:
Moles of Cl2 required = 2 * (moles of Ti)
Step 5: Determine the limiting reactant.
The limiting reactant is the reactant that is completely consumed, limiting the formation of the product.
To find the limiting reactant, compare the moles of each reactant to the required stoichiometric ratio.
If the moles of Cl2 required is greater than the moles of Cl2 given, then Cl2 is the limiting reactant.
If the moles of Cl2 required is less than the moles of Cl2 given, then Ti is the limiting reactant.
Step 6: Calculate the theoretical yield.
The theoretical yield is the maximum amount of product that can be formed from the limiting reactant. It is calculated based on the stoichiometric ratio and molar masses.
The molar mass of TiCl4 is 189.68 g/mol.
The moles of TiCl4 can be calculated using the moles of the limiting reactant:
Moles of TiCl4 = Moles of Ti * (Molar mass of TiCl4) / (molar mass of Ti)
The theoretical yield is calculated using the moles of TiCl4:
Theoretical yield = Moles of TiCl4 * Molar mass of TiCl4
Step 7: Calculate the percent yield.
Percent yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage.
Percent yield = (Actual yield / Theoretical yield) * 100
Given:
Mass of TiCl4 = 16.2 g
To find the theoretical yield, limiting reactant, and percent yield, follow these steps and use the given values in the calculations.