2. Find the mass in grams of $$ 2.00 imes 10^{23} $$ molecules of $$ F_{2} $$.

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2. Find the mass in grams of $$ 2.00 	imes 10^{23} $$ molecules of $$ F_{2} $$.

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To find the mass in grams of $$ 2.00 \times 10^{23} $$ molecules of $$ \text{F}_2 $$, follow these steps:

1. **Determine the Number of Moles:**
   
   Use Avogadro's number ($$ 6.022 \times 10^{23} $$ molecules/mol) to convert molecules to moles.
   
   $$
   \text{Number of moles} = \frac{2.00 \times 10^{23} \text{ molecules}}{6.022 \times 10^{23} \text{ molecules/mol}} \approx 0.332 \text{ mol}
   $$

2. **Calculate the Molar Mass of $$ \text{F}_2 $$:**
   
   Fluorine (F) has an atomic mass of approximately 19 g/mol. Therefore, the molar mass of $$ \text{F}_2 $$ is:
   
   $$
   \text{Molar mass of } \text{F}_2 = 2 \times 19 \text{ g/mol} = 38 \text{ g/mol}
   $$

3. **Find the Mass in Grams:**
   
   Multiply the number of moles by the molar mass to get the mass.
   
   $$
   \text{Mass} = 0.332 \text{ mol} \times 38 \text{ g/mol} \approx 12.6 \text{ g}
   $$

**Answer:**  
A mass of approximately 12.6 g of F₂ is present in 2.00 × 10²³ molecules.
The mass of $$ 2.00 \times 10^{23} $$ molecules of $$ \text{F}_2 $$ is approximately 12.6 grams.

2. Find the mass in grams of \( 2.00 \times 10^{23} \) molecules of \( F_{2} \).

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