How many grams of carbon are in 4.30×1023 molecules of (C3H5)2S?
To determine the number of grams of carbon in 4.30×10^23 molecules of (C3H5)2S, we need to calculate the molar mass of (C3H5)2S and then determine the mass of carbon within it.
Step 1: Calculate the molar mass of (C3H5)2S.
The molar mass of (C3H5)2S can be calculated by adding up the atomic masses of each element present (carbon, hydrogen, and sulfur).
- Carbon (C) has an atomic mass of 12.01 g/mol.
- Hydrogen (H) has an atomic mass of 1.01 g/mol.
- Sulfur (S) has an atomic mass of 32.07 g/mol.
Calculating the molar mass:
(3 * Atomic mass of Carbon) + (5 * Atomic mass of Hydrogen) + Atomic mass of Sulfur
= (3 * 12.01 g/mol) + (5 * 1.01 g/mol) + 32.07 g/mol
= 72.03 g/mol + 5.05 g/mol + 32.07 g/mol
= 109.15 g/mol
The molar mass of (C3H5)2S is 109.15 g/mol.
Step 2: Determine the mass of carbon.
Since each molecule of (C3H5)2S contains three carbon atoms, we can calculate the mass of carbon in one molecule by multiplying the molar mass of carbon by three.
Mass of carbon in one molecule = 3 * Atomic mass of Carbon
= 3 * 12.01 g/mol
= 36.03 g/mol
Step 3: Calculate the mass of carbon in 4.30×10^23 molecules.
Using Avogadro's number (6.022×10^23 molecules/mol), we can convert the number of molecules to moles and then calculate the mass of carbon.
Number of moles of (C3H5)2S = (4.30×10^23 molecules) / (6.022×10^23 molecules/mol)
= 0.713 mol
Mass of carbon = Number of moles of (C3H5)2S * Mass of carbon in one molecule
= 0.713 mol * 36.03 g/mol
= 25.73 g
Therefore, there are approximately 25.73 grams of carbon in 4.30×10^23 molecules of (C3H5)2S.