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Let's solve the problem step by step.

We are given:
- Mass of dry ice (solid CO₂): 0.050 g
- Volume of the container: 4.6 L
- Temperature: 86°F

We need to calculate the pressure inside the container once all the dry ice (CO₂) sublimates into gaseous form.

### Step 1: Convert the units
- **Mass**: We already have the mass in grams, but we need to convert it to moles using the molar mass of CO₂.
- **Temperature**: We need to convert from Fahrenheit to Kelvin.
- **Ideal gas law**: We will use the ideal gas law \( PV = nRT \).

### Molar mass of CO₂
CO₂ = \( 12.01 \, \text{g/mol} \) (C) + \( 2 \times 16.00 \, \text{g/mol} \) (O)
= 44.01 g/mol

Now, calculate the moles of CO₂:
\[
n = \frac{0.050 \, \text{g}}{44.01 \, \text{g/mol}} 
\]

### Step 2: Convert the temperature
The given temperature is 86°F. To use it in the ideal gas law, we need to convert it to Kelvin:

\[
T (K) = \left( \frac{86 - 32}{1.8} \right) + 273.15
\]

### Step 3: Apply the ideal gas law
The ideal gas law is:

\[
PV = nRT
\]

Where:
- \( P \) is the pressure (what we want to find),
- \( V \) is the volume (4.6 L),
- \( n \) is the number of moles,
- \( R \) is the gas constant = 0.0821 L·atm/(mol·K),
- \( T \) is the temperature in Kelvin.

Now let's calculate the result!The pressure inside the container after all the dry ice has sublimated into gaseous carbon dioxide is approximately 0.00615 atm.

Would you like further details or have any questions?

Here are 5 related questions to expand on this concept:
1. How does increasing the mass of dry ice affect the final pressure?
2. What would happen to the pressure if the temperature were lowered?
3. How is the ideal gas law affected by deviations from ideal gas behavior?
4. What would the pressure be if the volume of the container was halved?
5. How do you convert between different pressure units like atm, Pa, and mmHg?

**Tip:** When working with gases, always ensure that temperature is in Kelvin before applying the ideal gas law.

El hielo seco es dióxido de carbono sólido. Una muestra de 0.050 g de hielo seco se coloca en un recipiente vacío que tiene un volumen de 4.6 L a 86°F. Calcule la presión interior del recipiente después de que todo el hielo seco se ha convertido en dióxido de carbono gaseoso.

Learn how to calculate the pressure inside a 4.6 L container after 0.050 g of dry ice sublimates into gaseous carbon dioxide at 86°F. This problem involves applying the ideal gas law, converting units, and determining the moles of CO₂. Ideal for advanced high school or undergraduate chemistry students.

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