To determine the molecular mass of sulfuric acid [tex]\( H_2SO_4 \)[/tex], we'll follow these steps:
1. Identify the atomic masses of the elements involved:
- Hydrogen ([tex]\(H\)[/tex]): [tex]\(0.00101 \, \text{kg/mol}\)[/tex]
- Sulfur ([tex]\(S\)[/tex]): [tex]\(0.0321 \, \text{kg/mol}\)[/tex]
- Oxygen ([tex]\(O\)[/tex]): [tex]\(0.0160 \, \text{kg/mol}\)[/tex]
2. Determine the number of atoms of each element in the sulfuric acid molecule [tex]\( H_2SO_4 \)[/tex]:
- [tex]\(H\)[/tex]: 2 atoms
- [tex]\(S\)[/tex]: 1 atom
- [tex]\(O\)[/tex]: 4 atoms
3. Calculate the contribution of each element to the molecular mass of sulfuric acid:
- Contribution from hydrogen: [tex]\(2 \times 0.00101 \, \text{kg/mol} = 0.00202 \, \text{kg/mol}\)[/tex]
- Contribution from sulfur: [tex]\(1 \times 0.0321 \, \text{kg/mol} = 0.0321 \, \text{kg/mol}\)[/tex]
- Contribution from oxygen: [tex]\(4 \times 0.0160 \, \text{kg/mol} = 0.0640 \, \text{kg/mol}\)[/tex]
4. Sum the contributions for the total molecular mass:
[tex]\[
\text{Molecular mass of } H_2SO_4 = 0.00202 \, \text{kg/mol} + 0.0321 \, \text{kg/mol} + 0.0640 \, \text{kg/mol} = 0.09812 \, \text{kg/mol}
\][/tex]
Thus, the molecular mass of sulfuric acid [tex]\( H_2SO_4 \)[/tex] is [tex]\(0.09812 \, \text{kg/mol}\)[/tex].
