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The problem presented involves determining the number of moles of a gaseous compound with the empirical formula \( SF_4 \). Let's break down the data and use the **ideal gas law** equation:

\[
PV = nRT
\]

where:
- \( P \) = pressure = 1.02 atm
- \( V \) = volume = 22.1 mL = 0.0221 L (since 1000 mL = 1 L)
- \( n \) = moles of gas (what we want to find)
- \( R \) = ideal gas constant = 0.0821 L·atm/(mol·K)
- \( T \) = temperature = 20°C = 293.15 K (by adding 273.15 to Celsius)

### Step 1: Solve for moles (\(n\)) using the ideal gas law.

Rearrange the ideal gas law to solve for \(n\):

\[
n = \frac{PV}{RT}
\]

Substitute the known values into the equation:

\[
n = \frac{(1.02 \, \text{atm}) \times (0.0221 \, \text{L})}{(0.0821 \, \text{L·atm/(mol·K)}) \times (293.15 \, \text{K})}
\]

Now, let's calculate the value of \(n\).The number of moles of the compound present is approximately \( 9.37 \times 10^{-4} \) moles.

Would you like more details or have any questions?

Here are some related questions:
1. How would the result change if the temperature was 25°C instead of 20°C?
2. How can we calculate the molecular weight of \( SF_4 \) using its mass and moles?
3. What assumptions are made when using the ideal gas law?
4. How would the result differ if the pressure was reduced to 0.98 atm?
5. How does the molar mass of \( SF_4 \) affect the result in practical applications?

**Tip:** Always convert temperatures to Kelvin when applying the ideal gas law.

Un compuesto tiene la fórmula empírica SF_4. A 20°C, 0.1 g del compuesto gaseoso ocupan un volumen de 22.1 mL y ejercen una presión de 1.02 atm. ¿Cuántas moles del compuesto están presente?

Resuelve el cálculo de moles de un compuesto gaseoso SF_4 usando la ley de gases ideales. Se te proporcionan los valores de presión, volumen y temperatura para encontrar la cantidad de moles. Aprende los conceptos de conversión de unidades y el uso de la ley de gases ideales. Adecuado para estudiantes de nivel secundaria superior.

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