I need help please??
Calculate the empirical formula for a compound composed of 13.27g Carbon and 70.9g sulfur.
I got C1S2. Is this correct?
Yes. You have 1.05 moles C, 2.10 moles S
CS2
To calculate the empirical formula, you need to determine the ratio of different elements in a compound. Let's go through the steps together:
Step 1: Convert the mass of each element to moles.
- Carbon (C): You have 13.27g. The molar mass of carbon is approximately 12.01 g/mol, so you can use the following equation to convert grams to moles: moles = mass/molar mass.
moles of carbon = 13.27g / 12.01 g/mol ≈ 1.10 mol
- Sulfur (S): You have 70.9g. The molar mass of sulfur is approximately 32.07 g/mol, so you can use the same equation to convert grams to moles.
moles of sulfur = 70.9g / 32.07 g/mol ≈ 2.21 mol
Step 2: Divide the number of moles of each element by the smallest number of moles.
- In this case, the smallest number of moles is approximately 1.10 mol (from carbon).
- Divide the number of moles of each element by 1.10 mol:
moles of carbon ≈ 1.10 mol / 1.10 mol = 1 mol
moles of sulfur ≈ 2.21 mol / 1.10 mol ≈ 2 mol
Step 3: Find the whole number ratio of elements.
- From the above calculation, the empirical formula becomes C1S2.
Based on the calculations, your empirical formula C1S2 is not correct. The correct empirical formula for the compound composed of 13.27g carbon and 70.9g sulfur is CS2.