In an industrial process, the following reaction is carried out in the presence of a catalyst:

C2H51 + Cl2 → C2H51Cl12

Calculate the percentage yield if 405.58 grams of C2H51 are used in the reaction and 474.91 grams of C2H51Cl12 are produced.

Follow these steps.

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To calculate the percentage yield of a reaction, you need to compare the actual yield (the amount of product obtained experimentally) to the theoretical yield (the maximum amount of product that can be obtained based on stoichiometry).

To determine the theoretical yield, you first need to balance the equation:
C2H51 + Cl2 → C2H51Cl12

From the balanced equation, it can be seen that the stoichiometric ratio between C2H51 and C2H51Cl12 is 1:1. This means that the reaction ratio is 1 mole of C2H51 to 1 mole of C2H51Cl12.

Next, you need to convert the given masses of C2H51 and C2H51Cl12 to moles using their respective molar masses.

The molar mass of C2H51 is calculated as follows:
2 * molar mass of C (12.01 g/mol) + 5 * molar mass of H (1.01 g/mol) = 58.13 g/mol

For 405.58 grams of C2H51:
405.58 g / 58.13 g/mol = 6.98 mol

The molar mass of C2H51Cl12 is calculated as follows:
2 * molar mass of C (12.01 g/mol) + 5 * molar mass of H (1.01 g/mol) + 12 * molar mass of Cl (35.45 g/mol) = 181.04 g/mol

For 474.91 grams of C2H51Cl12:
474.91 g / 181.04 g/mol = 2.62 mol

Since the reaction ratio is 1:1, the theoretical yield of C2H51Cl12 is 6.98 moles.

To calculate the percentage yield, divide the actual yield (mass of C2H51Cl12 obtained) by the theoretical yield (mass of C2H51Cl12 calculated) and multiply by 100:

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

Percentage Yield = (474.91 g / (2.62 mol * 181.04 g/mol)) * 100

Percentage Yield = 85.6%

Therefore, the percentage yield of the reaction is approximately 85.6%.