0.063 g of F2 react with excess Na by the equation below. Determine the number of molecules of of NaF that can be produced. Express your answer in scientific notation using the format (for example) 6.022*10^23 for 6.022 x 1023.

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

Let's solve this step by step to find the number of molecules of NaF that can be produced from 0.063 g of F₂.

### Step 1: Molar mass of F₂
First, we calculate the molar mass of F₂ (fluorine gas):

- The atomic mass of fluorine (F) is approximately 19.00 g/mol.
- Molar mass of F₂ = 2 × 19.00 = **38.00 g/mol**.

### Step 2: Convert grams of F₂ to moles
Now, we convert the given mass of F₂ to moles using the molar mass:

\[
\text{moles of F}_2 = \frac{\text{mass of F}_2}{\text{molar mass of F}_2} = \frac{0.063\ \text{g}}{38.00\ \text{g/mol}} = 1.66 \times 10^{-3}\ \text{mol}
\]

### Step 3: Use stoichiometry to find moles of NaF
From the balanced chemical equation:

\[
2\text{Na}(s) + \text{F}_2(g) \rightarrow 2\text{NaF}(s)
\]

This equation shows that 1 mole of F₂ produces 2 moles of NaF. Therefore, the moles of NaF produced will be:

\[
\text{moles of NaF} = 2 \times \text{moles of F}_2 = 2 \times (1.66 \times 10^{-3}\ \text{mol}) = 3.32 \times 10^{-3}\ \text{mol}
\]

### Step 4: Convert moles of NaF to molecules
Next, we convert the moles of NaF to the number of molecules using Avogadro's number, which is \(6.022 \times 10^{23}\ \text{molecules/mol}\):

\[
\text{molecules of NaF} = 3.32 \times 10^{-3}\ \text{mol} \times 6.022 \times 10^{23}\ \text{molecules/mol}
\]

\[
\text{molecules of NaF} = 2.00 \times 10^{21}\ \text{molecules}
\]

### Final Answer:
The number of molecules of NaF that can be produced is **2.00 × 10²¹** molecules.

---

Would you like further details or have any questions? Here are some related questions:

1. What is the relationship between moles of reactants and products in a balanced chemical equation?
2. How does the concept of limiting reactant affect the number of products produced?
3. How do you convert between moles and molecules?
4. How do you calculate the molar mass of a compound like NaF?
5. What is Avogadro’s number, and why is it important in chemistry?

**Tip:** Always ensure you balance the chemical equation first before using stoichiometry to relate reactants and products!

0.063 g of F2 react with excess Na by the equation below. Determine the number of molecules of NaF that can be produced. Express your answer in scientific notation using the format (for example) 6.022*10^23 for 6.022 x 1023.

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

Learn how to calculate the number of NaF molecules produced from 0.063g of F2. This step-by-step solution covers key concepts in stoichiometry, molar mass calculations, and mole-to-molecule conversions using Avogadro's number. Suitable for high school chemistry students (Grades 10-12).

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation