Find the molecular mass of sulphuric acid
The Correct Answer and Explanation is:
The molecular mass of sulfuric acid (H₂SO₄) can be calculated by adding the atomic masses of all the atoms in the molecule.
Step-by-step calculation:
- Hydrogen (H):
- There are 2 hydrogen atoms in H₂SO₄. The atomic mass of hydrogen is 1 g/mol.
- Contribution to the molecular mass: 2×1=22 \times 1 = 22×1=2 g/mol.
- Sulfur (S):
- There is 1 sulfur atom in H₂SO₄. The atomic mass of sulfur is 32 g/mol.
- Contribution to the molecular mass: 1×32=321 \times 32 = 321×32=32 g/mol.
- Oxygen (O):
- There are 4 oxygen atoms in H₂SO₄. The atomic mass of oxygen is 16 g/mol.
- Contribution to the molecular mass: 4×16=644 \times 16 = 644×16=64 g/mol.
Adding them all together:
- 2 g/mol (H)+32 g/mol (S)+64 g/mol (O)=98 g/mol2 \, \text{g/mol} \, (\text{H}) + 32 \, \text{g/mol} \, (\text{S}) + 64 \, \text{g/mol} \, (\text{O}) = 98 \, \text{g/mol}2g/mol(H)+32g/mol(S)+64g/mol(O)=98g/mol.
Therefore, the molecular mass of sulfuric acid (H₂SO₄) is 98 g/mol.
Explanation:
The molecular mass is essentially the sum of the atomic masses of the atoms present in the molecule. Since sulfuric acid consists of two hydrogen atoms, one sulfur atom, and four oxygen atoms, we simply multiply the number of each atom by its respective atomic mass and then sum the values. This gives the molecular mass, which is crucial in determining the amount of the compound in a given quantity or solution, especially in calculations related to molarity or stoichiometry. The molecular mass also plays a key role in understanding the chemical behavior and reactivity of the compound.
