Final answer:
The actual yield of carbon tetrachloride when 100 g of carbon disulfide reacts with 100 g of chlorine, given a 90.0% yield, is 64.99 g.
Step-by-step explanation:
Calculation of Actual Yield of Carbon Tetrachloride
To calculate the actual yield of carbon tetrachloride when carbon disulfide reacts with chlorine, it is important first to identify the limiting reactant and then use the stoichiometry of the balanced equation to find the theoretical yield. From there, we can use the percentage yield to find the actual yield of the product.
The balanced equation is:
CS₂ + 3Cl₂ → CCl₄ + S₂Cl₂
Molecular masses:
CS₂ = 76.2 g/mol,
Cl₂ = 71.0 g/mol,
CCl₄ = 154 g/mol.
Using the provided masses of 100 g of CS₂ and 100 g of Cl₂, we first convert these masses to moles:
- Moles of CS₂ = 100 g / 76.2 g/mol = 1.312 moles
- Moles of Cl₂ = 100 g / 71.0 g/mol = 1.408 moles
The stoichiometry of the reaction shows that 1 mole of CS₂ reacts with 3 moles of Cl₂. Thus, Cl₂ is the limiting reactant, as we don't have enough (3 moles for every 1 mole of CS₂).
Now, we calculate the theoretical yield of CCl₄ based on the limiting reagent (Cl₂).
- Moles of CCl₄ produced = Moles of Cl₂ / 3 = 1.408 moles / 3 = 0.469 moles
- Mass of CCl₄ (theoretical yield) = 0.469 moles * 154 g/mol = 72.23 g
Given a 90.0% percent yield, the actual yield can be calculated as follows:
- Actual yield = Theoretical yield * (Percentage yield / 100) = 72.23 g * (90.0 / 100) = 64.99 g
The actual yield of CCl₄ in this reaction, given a 90.0% yield, is 64.99 g.