Answer :
To find the molar mass of sulfuric acid, $\mathrm{H_2SO_4}$, we must add the masses of all the atoms in one mole of the compound. The molecule consists of:
- 2 hydrogen atoms,
- 1 sulfur atom, and
- 4 oxygen atoms.
The atomic masses are given as:
- Hydrogen: $1.01\ \mathrm{g/mol}$
- Sulfur: $32.07\ \mathrm{g/mol}$
- Oxygen: $16.00\ \mathrm{g/mol}$
First, calculate the mass contributed by each element:
1. For hydrogen:
$$\text{Mass of H} = 2 \times 1.01\ \mathrm{g/mol} = 2.02\ \mathrm{g/mol}$$
2. For sulfur:
$$\text{Mass of S} = 1 \times 32.07\ \mathrm{g/mol} = 32.07\ \mathrm{g/mol}$$
3. For oxygen:
$$\text{Mass of O} = 4 \times 16.00\ \mathrm{g/mol} = 64.00\ \mathrm{g/mol}$$
Now, add these contributions to get the total molar mass:
$$
\text{Molar mass of } \mathrm{H_2SO_4} = 2.02 + 32.07 + 64.00 = 98.09\ \mathrm{g/mol}
$$
Thus, the molar mass of $\mathrm{H_2SO_4}$ is approximately $98.1\ \mathrm{grams}$.
- 2 hydrogen atoms,
- 1 sulfur atom, and
- 4 oxygen atoms.
The atomic masses are given as:
- Hydrogen: $1.01\ \mathrm{g/mol}$
- Sulfur: $32.07\ \mathrm{g/mol}$
- Oxygen: $16.00\ \mathrm{g/mol}$
First, calculate the mass contributed by each element:
1. For hydrogen:
$$\text{Mass of H} = 2 \times 1.01\ \mathrm{g/mol} = 2.02\ \mathrm{g/mol}$$
2. For sulfur:
$$\text{Mass of S} = 1 \times 32.07\ \mathrm{g/mol} = 32.07\ \mathrm{g/mol}$$
3. For oxygen:
$$\text{Mass of O} = 4 \times 16.00\ \mathrm{g/mol} = 64.00\ \mathrm{g/mol}$$
Now, add these contributions to get the total molar mass:
$$
\text{Molar mass of } \mathrm{H_2SO_4} = 2.02 + 32.07 + 64.00 = 98.09\ \mathrm{g/mol}
$$
Thus, the molar mass of $\mathrm{H_2SO_4}$ is approximately $98.1\ \mathrm{grams}$.
