High School

C₆H₆ + Cl₂ → C₆H₅Cl + HCl

When 36.8 g of C₆H₆ reacts with an excess of chlorine, the actual yield of C₆H₅Cl is 38.8 g.

What is the percent yield and percent error of C₆H₅Cl?

Answer :

To calculate percent yield and percent error, first determine the theoretical yield from the balanced equation and given starting material. The percent yield is found to be 73.18%, and the percent error is 26.82%. These calculations provide insight into reaction efficiency.

To determine the percent yield and percent error, follow these steps:

Step 1: Calculate Theoretical Yield

The balanced equation is:

C₆H₆ + Cl₂ --> C₆H₅Cl + HCl

Molar masses are: C₆H₆ (78.11 g/mol) and C₆H₅Cl (112.56 g/mol)

Moles of C₆H₆ = 36.8 g / 78.11 g/mol = 0.471 moles.

Theoretical yield of C₆H₅Cl = 0.471 moles * 112.56 g/mol = 53.03 g.

Step 2: Calculate Percent Yield

Percent Yield = (Actual Yield / Theoretical Yield) * 100

Percent Yield = (38.8 g / 53.03 g) * 100 = 73.18%

Step 3: Calculate Percent Error

Percent Error = |(Theoretical Yield - Actual Yield) / Theoretical Yield| * 100

Percent Error = |(53.03 g - 38.8 g) / 53.03 g| * 100 = 26.82%

Therefore, the percent yield of C₆H₅Cl is 73.18% and the percent error is 26.82%.