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To solve this problem, we need to:

1. **Calculate the number of moles** of sulfur hexafluoride (SF₆) and chlorine pentafluoride (ClF₅).
2. **Find the mole fraction** of each gas.
3. **Determine the partial pressure** of each gas using the ideal gas law.
4. **Calculate the total pressure** in the tank.

### Step 1: Calculate the number of moles
The number of moles of a substance can be found using:
\[
n = \frac{\text{mass}}{\text{molar mass}}
\]

- **Molar mass of SF₆**: 146.06 g/mol
- **Molar mass of ClF₅**: 130.44 g/mol

- Mass of SF₆: 2.53 g
- Mass of ClF₅: 12.7 g

#### Number of moles of SF₆:
\[
n_{SF₆} = \frac{2.53 \, \text{g}}{146.06 \, \text{g/mol}}
\]

#### Number of moles of ClF₅:
\[
n_{ClF₅} = \frac{12.7 \, \text{g}}{130.44 \, \text{g/mol}}
\]

### Step 2: Mole Fraction
The mole fraction of a gas is calculated as:
\[
\text{Mole fraction of gas A} = \frac{n_A}{n_{\text{total}}}
\]
Where \(n_{\text{total}} = n_{SF₆} + n_{ClF₅}\).

### Step 3: Partial Pressure using Ideal Gas Law
The partial pressure of each gas is found using the ideal gas law:
\[
P = \frac{nRT}{V}
\]
Where:
- \(P\) is the pressure (in atm),
- \(n\) is the number of moles,
- \(R\) is the ideal gas constant (0.0821 L·atm/(mol·K)),
- \(T\) is the temperature in Kelvin (0.22 °C = 273.37 K),
- \(V\) is the volume (6.00 L).

We'll now compute these values.Here are the results for the given problem:

- **Mole fraction of sulfur hexafluoride (SF₆)**: 0.151
- **Partial pressure of SF₆**: 0.065 atm
- **Mole fraction of chlorine pentafluoride (ClF₅)**: 0.849
- **Partial pressure of ClF₅**: 0.364 atm
- **Total pressure in the tank**: 0.429 atm

Would you like any additional details or further clarification on any of the steps?

### Related questions:
1. How is the ideal gas law used to calculate pressure in a real-life scenario?
2. What are the assumptions made for gases behaving ideally?
3. How would the solution change if the gases were non-ideal?
4. Can you calculate the volume if the pressure and temperature are given?
5. What is the relationship between partial pressure and mole fraction in a gas mixture?

### Tip:
When calculating gas mixtures, remember that the sum of all mole fractions in the mixture will always equal 1.

A 6.00 L tank at 0.22°C is filled with 2.53 g of sulfur hexafluoride and 12.7 g of chlorine pentafluoride. Calculate the mole fraction, partial pressure of each gas, and total pressure assuming both gases behave as ideal gases.

Solve a gas mixture problem involving 2.53 g of sulfur hexafluoride and 12.7 g of chlorine pentafluoride in a 6.00 L tank at 0.22°C. This problem covers the calculation of mole fractions, partial pressures, and total pressure using the ideal gas law. Ideal for undergraduate chemistry students.

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