2.71 x 1022 moleciules of F2 react with excess Na by the equation below. Determine the mass of of NaF that can be produced.

2Na(s) + F2(g) -> 2NaF(s)

To determine the mass of NaF produced, we'll follow these steps:

1. **Find the moles of F2**:  
   The given number of molecules of F2 is \(2.71 \times 10^{22}\).  
   To convert molecules to moles, we use Avogadro's number (\(6.022 \times 10^{23}\) molecules per mole).

   \[
   \text{Moles of } F_2 = \frac{2.71 \times 10^{22} \, \text{molecules}}{6.022 \times 10^{23} \, \text{molecules/mol}} = 0.045 \, \text{mol of } F_2
   \]

2. **Use the stoichiometry of the reaction**:  
   According to the balanced chemical equation:  
   \[
   2Na(s) + F_2(g) \rightarrow 2NaF(s)
   \]
   The ratio of Na to F2 is 2:1, meaning 1 mole of F2 reacts with 2 moles of Na to produce 2 moles of NaF.

3. **Calculate moles of NaF produced**:  
   From the stoichiometry, 1 mole of F2 produces 2 moles of NaF.  
   Therefore, \(0.045 \, \text{mol of } F_2\) will produce:  
   \[
   0.045 \, \text{mol} \, F_2 \times 2 = 0.090 \, \text{mol of NaF}
   \]

4. **Calculate the mass of NaF**:  
   The molar mass of NaF is the sum of the atomic masses of Na (22.99 g/mol) and F (18.998 g/mol):  
   \[
   \text{Molar mass of NaF} = 22.99 + 18.998 = 41.988 \, \text{g/mol}
   \]
   Now, calculate the mass of NaF:  
   \[
   \text{Mass of NaF} = 0.090 \, \text{mol} \times 41.988 \, \text{g/mol} = 3.779 \, \text{g}
   \]

**Answer**: The mass of NaF that can be produced is approximately 3.78 grams.

Would you like further explanation or details on any of the steps? Here are some related questions:

1. How does Avogadro's number relate to mole calculations?
2. What is the significance of stoichiometry in balancing chemical reactions?
3. How do you convert between moles and mass in chemistry?
4. What other compounds can be formed from Na and F?
5. How do you determine the limiting reactant in chemical reactions?

**Tip**: Always ensure your units are consistent when performing stoichiometric calculations.

2.71 x 10^22 molecules of F2 react with excess Na by the equation below. Determine the mass of NaF that can be produced. 

2Na(s) + F2(g) -> 2NaF(s)

Learn how to calculate the mass of NaF produced when 2.71 x 10^22 molecules of F2 react with excess Na. This step-by-step solution involves mole calculations, stoichiometry, and mass-mole conversions, with a detailed explanation of the key formulas used. Suitable for high school chemistry students.

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