How many grams of C17H15 are in a sample containing 6.003 x 1024 molecules?

To find the number of grams of \( C_{17}H_{15} \) (a molecule containing 17 carbon and 15 hydrogen atoms), we need to follow these steps:

### Step 1: Use Avogadro's Number
Avogadro’s number is \( 6.022 \times 10^{23} \) molecules per mole. This allows us to determine how many moles correspond to the given number of molecules.

\[
\text{Number of moles} = \frac{6.003 \times 10^{24} \, \text{molecules}}{6.022 \times 10^{23} \, \text{molecules/mol}}
\]

\[
\text{Number of moles} = 9.97 \, \text{mol}
\]

### Step 2: Calculate the Molar Mass of \( C_{17}H_{15} \)
The molar mass is calculated as:

\[
(17 \times 12.01 \, \text{g/mol}) + (15 \times 1.008 \, \text{g/mol})
\]

\[
= 204.17 \, \text{g/mol} + 15.12 \, \text{g/mol} = 219.29 \, \text{g/mol}
\]

### Step 3: Calculate the Mass of the Sample
Using the number of moles and the molar mass:

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

\[
\text{Mass} = 9.97 \, \text{mol} \times 219.29 \, \text{g/mol} = 2187.9 \, \text{g}
\]

### Final Answer
The mass of the sample is approximately:

\[
2187.9 \, \text{grams}
\]

Would you like a deeper breakdown or have additional questions?

---

1. What is Avogadro's number and its significance in chemistry?  
2. How do you find the molar mass of any compound?  
3. What are moles, and why are they important?  
4. Can you calculate mass if only volume and density are given?  
5. How does molecular structure affect a compound’s mass?

**Tip:** Memorizing atomic masses of key elements like C (12.01 g/mol) and H (1.008 g/mol) can speed up calculations.

How many grams of C17H15 are in a sample containing 6.003 x 10^24 molecules?

Learn how to calculate the mass of a sample containing 6.003 x 10^24 molecules of C17H15. This problem covers Avogadro's number, molar mass, and mole calculations, providing a step-by-step solution. Suitable for high school students in Grades 11-12.

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