What is the percent by weight of Cl in DDT, C14H9Cl5?

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BlackTom AI · Accepted Answer

Question restatement: What is the percent by weight of Cl in DDT, with the formula C14H9Cl5?

Option provided: a. 50.0%

Step-by-step reasoning regarding the calculation: First, determine the molecular formula and count the atoms: DDT consists of 14 carbons (C), 9 hydrogens (H), and 5 chlorines (Cl). To find the mass percent of chlorine, we need the molar masses: carbon ≈ 12.01 g/mol, hydrogen ≈ 1.008 g/mol, chlorine ≈ 35.45 g/mol.

Next, compute the total molar mass: carbon contribution = 14 × 12.01 ≈ 168.14 g/mol; hydrogen contribution = 9 × 1.008 ≈ 9.07 g/mol; chlorine contribution = 5 × 35.45 ≈ 177.25 g/mol. Sum = 168.14 + 9.07 + 177.25 ≈ 354.46 g/mol.

Then, determine the mass fraction of chlorine: chlorine mass = 177.25 g/mol divided by the total molar mass 354.46 g/mol, which equals approximately 0.500 (50.0%). Convert to a percentage by multiplying by 100: 50.0% Cl by weight.

Notes on potential sources of error: if different atomic masses are used (slightly different standard values), you might get a result very close to 50%, but using standard atomic masses around 12.01 (C), 1.008 (H), and 35.45 (Cl) yields the 50% figure.

Why this aligns with the concept: mass percent is defined as (mass of element in one mole of compound) / (molar mass of compound) × 100%; for DDT, the chlorine contribution constitutes about half of the compound’s mass due to 5 Cl atoms contributing a large mass relative to the rest.

If one were to evaluate other possible options, they would need to reflect deviations from this calculation, such as using a different molar mass for chlorine or miscounting the number of chlorine atoms, which would shift the percent Cl away from 50%.

MUF0041 Chemistry Unit 1 - Semester 1, 2025 2.12 Quiz: Percentage Composition and Empirical Formula

What is the percent by weight of Cl in DDT, C14H9Cl5?

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