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The problem asks to calculate the pressure of sulfur hexafluoride (\(\text{SF}_6\)) gas after a reaction, given the following information:

- Temperature: 32.0°C (which is 305.15 K when converted to Kelvin),
- Volume: 4.00 L,
- Mass of \(\text{SF}_6\): 24.0 g.

We will use the ideal gas law equation: 

\[
PV = nRT
\]

Where:
- \(P\) is the pressure (in atm),
- \(V\) is the volume (in liters),
- \(n\) is the number of moles of gas,
- \(R\) is the ideal gas constant, \(R = 0.0821 \, \text{L·atm·mol}^{-1} \text{K}^{-1}\),
- \(T\) is the temperature in Kelvin.

### Step 1: Convert the mass of \(\text{SF}_6\) to moles

The molar mass of \(\text{SF}_6\) is calculated as follows:

\[
\text{Molar mass of } \text{SF}_6 = 32.07 \, (\text{S}) + 6 \times 18.998 \, (\text{F}) = 146.06 \, \text{g/mol}
\]

Now, convert 24.0 g of \(\text{SF}_6\) to moles:

\[
n = \frac{\text{mass}}{\text{molar mass}} = \frac{24.0 \, \text{g}}{146.06 \, \text{g/mol}} = 0.1643 \, \text{mol}
\]

### Step 2: Rearrange the ideal gas law to solve for pressure \(P\)

\[
P = \frac{nRT}{V}
\]

Substitute the known values:

\[
P = \frac{(0.1643 \, \text{mol})(0.0821 \, \text{L·atm·mol}^{-1} \text{K}^{-1})(305.15 \, \text{K})}{4.00 \, \text{L}}
\]

### Step 3: Calculate the pressure

\[
P = \frac{(4.1157)}{4.00} = 1.0289 \, \text{atm}
\]

### Final Answer:
The pressure of sulfur hexafluoride gas in the reaction vessel is **1.03 atm** (rounded to three significant figures).

Would you like more details or have any questions about the steps?

### 5 Related Questions:
1. How is the ideal gas law applied in real-life chemical reactions?
2. What happens if the temperature of the reaction vessel increases?
3. Can the ideal gas law be used for gases that do not behave ideally?
4. How does the volume of the container affect the pressure of a gas?
5. Why is it important to convert Celsius to Kelvin in gas law calculations?

### Tip:
Always ensure to convert temperatures to Kelvin when using the ideal gas law because the Kelvin scale starts at absolute zero, ensuring the calculations remain consistent.

A reaction between liquid reactants takes place at 32.0°C in a sealed, evacuated vessel with a measured volume of 4.00 L. Measurements show that the reaction produced 24.0 g of sulfur hexafluoride gas. Calculate the pressure of sulfur hexafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits.

Learn how to calculate the pressure of sulfur hexafluoride gas produced in a sealed reaction vessel at 32.0°C with a volume of 4.00 L. This detailed solution applies the ideal gas law and stoichiometry, using the formula PV = nRT. Suitable for high school students in Grades 11-12.

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