The empirical formula of the compound with 15.8 % Carbon (C) and 84.2% Sulfur (S)Select one Question 10Answera.CS4b.CS2c.CSd.CS3

Break Down the Problem

1. Identify the percent composition of each element in the compound.
2. Convert the percentages to moles by using the molar mass of each element.
3. Determine the simplest whole number ratio of moles of the elements.

Relevant Concepts

• Molar mass of Carbon (C) = 12.01 g/mol
• Molar mass of Sulfur (S) = 32.07 g/mol

Analysis and Detail

1. Calculate moles of Carbon: $\text{Moles of C} = \frac{15.8 \, \text{g}}{12.01 \, \text{g/mol}} \approx 1.32 \, \text{mol}$

2. Calculate moles of Sulfur: $\text{Moles of S} = \frac{84.2 \, \text{g}}{32.07 \, \text{g/mol}} \approx 2.62 \, \text{mol}$

3. Determine the ratio of moles of C to S:

   • Divide both values by the smallest number of moles calculated (1.32): $\text{Ratio of C} = \frac{1.32}{1.32} = 1$ $\text{Ratio of S} = \frac{2.62}{1.32} \approx 1.98 \approx 2$

Verify and Summarize

The simplest whole number ratio of the elements is approximately:

• C : S = 1 : 2

Final Answer

The empirical formula of the compound is CS₂. Therefore, the correct answer is b. CS₂.