To find the mass of \( 0.15 \, \text{mol} \) of \( \text{H}_2\text{SO}_4 \) (sulfuric acid), we can use the formula:

\[
\text{Mass} = \text{Moles} \times \text{Molar Mass}
\]

1. **Calculate the molar mass of \( \text{H}_2\text{SO}_4 \):**
   - Hydrogen (\( \text{H} \)): \( 2 \times 1 = 2 \, \text{g/mol} \)
   - Sulfur (\( \text{S} \)): \( 1 \times 32 = 32 \, \text{g/mol} \)
   - Oxygen (\( \text{O} \)): \( 4 \times 16 = 64 \, \text{g/mol} \)
   
   Adding these together gives:
   \[
   \text{Molar Mass of } \text{H}_2\text{SO}_4 = 2 + 32 + 64 = 98 \, \text{g/mol}
   \]

2. **Calculate the mass:**
   \[
   \text{Mass} = 0.15 \, \text{mol} \times 98 \, \text{g/mol} = 14.7 \, \text{g}
   \]

So, \( 0.15 \, \text{mol} \) of \( \text{H}_2\text{SO}_4 \) has a mass of **14.7 grams**.

Would you like more details, or have any questions?

Here are five related questions to expand your understanding:

1. How would the mass change if we had \( 0.25 \, \text{mol} \) of \( \text{H}_2\text{SO}_4 \)?
2. What is the volume of \( 0.15 \, \text{mol} \) of \( \text{H}_2\text{SO}_4 \) solution with a given concentration?
3. How do you determine the molar mass of a compound with different elements?
4. What mass would 1 mole of \( \text{H}_2\text{SO}_4 \) occupy in a solid form?
5. How would you calculate the number of molecules in \( 0.15 \, \text{mol} \) of \( \text{H}_2\text{SO}_4 \)?

**Tip:** Always verify each element's atomic mass from the periodic table when calculating molar masses.

Learn how to find the mass of 0.15 mol of sulfuric acid (H₂SO₄) using molar mass calculations. This step-by-step solution provides insight into stoichiometry and key chemistry concepts. Perfect for high school students in Grades 10-12.

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