H_(2)SO_(4) Solve for the molar mass of the following compounds. Make sure and show your work and don't forget to put your unit.

To calculate the molar mass of \( H_2SO_4 \) (sulfuric acid), we need to sum up the atomic masses of all the atoms present in the compound. The molecular formula \( H_2SO_4 \) indicates that it contains:<br /><br />- 2 hydrogen (H) atoms<br />- 1 sulfur (S) atom<br />- 4 oxygen (O) atoms<br /><br />We will use the following approximate atomic masses for each element:<br /><br />- Hydrogen (H): 1.01 g/mol<br />- Sulfur (S): 32.07 g/mol<br />- Oxygen (O): 16.00 g/mol<br /><br />Now, let's calculate the molar mass step by step:<br /><br />1. Calculate the total mass of hydrogen:<br /> \[<br /> 2 \times 1.01 \, \text{g/mol} = 2.02 \, \text{g/mol}<br /> \]<br /><br />2. Calculate the total mass of sulfur:<br /> \[<br /> 1 \times 32.07 \, \text{g/mol} = 32.07 \, \text{g/mol}<br /> \]<br /><br />3. Calculate the total mass of oxygen:<br /> \[<br /> 4 \times 16.00 \, \text{g/mol} = 64.00 \, \text{g/mol}<br /> \]<br /><br />4. Add up all the masses to find the molar mass of \( H_2SO_4 \):<br /> \[<br /> 2.02 \, \text{g/mol} + 32.07 \, \text{g/mol} + 64.00 \, \text{g/mol} = 98.09 \, \text{g/mol}<br /> \]<br /><br />Therefore, the molar mass of \( H_2SO_4 \) is \( 98.09 \, \text{g/mol} \).