A sample of a gas mixture contains the following quantities of three gases. compound mass CO 1.08 g CO2 1.84 g SF6 1.54 g The sample has: volume = 2.50 L temperature - 16.6 °C What is the partial pressure for each gas, in mmHg? What is the total pressure in the flask? CO mmHg CO2 mmHg SF6 mmHg total mmHg Submit Show Approach Hide Tutor Steps

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Chapter1: Chemical Foundations
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### Gas Mixture Sample Problem

A sample of a gas mixture contains the following quantities of three gases:

| Compound | Mass  |
|----------|-------|
| CO       | 1.08 g|
| CO₂      | 1.84 g|
| SF₆      | 1.54 g|

#### Sample Conditions:
- **Volume**: 2.50 L
- **Temperature**: 16.6°C

### Task
Determine the partial pressure for each gas in mmHg and the total pressure in the flask.

### Formulae Needed:

You will need the ideal gas law, which is stated as:
\[ PV = nRT \]
where:
- \( P \) = pressure (in atm)
- \( V \) = volume (in liters)
- \( n \) = number of moles
- \( R \) = ideal gas constant (0.0821 L·atm·K⁻¹·mol⁻¹)
- \( T \) = temperature (in Kelvin) 

**Note:** Convert temperature to Kelvin by using \( T(K) = T(°C) + 273.15 \).

### Steps to Complete:
1. Convert the temperature from Celsius to Kelvin.
2. Calculate the moles of each gas using their respective masses and molar masses.
3. Use the ideal gas law to find the partial pressure of each gas.
4. Sum the partial pressures to find the total pressure in the flask.

### Input Fields:
- CO: _______ mmHg
- CO₂: _______ mmHg
- SF₆: _______ mmHg
- Total: _______ mmHg

### Interactive Elements:
- **Buttons**: `Submit`, `Show Approach`, `Hide Tutor Steps`

Make sure to fill out the pressure values in the corresponding input fields to check your results. The `Show Approach` and `Hide Tutor Steps` buttons can help you understand the method to solve this problem or hide the guiding steps if needed.
Transcribed Image Text:### Gas Mixture Sample Problem A sample of a gas mixture contains the following quantities of three gases: | Compound | Mass | |----------|-------| | CO | 1.08 g| | CO₂ | 1.84 g| | SF₆ | 1.54 g| #### Sample Conditions: - **Volume**: 2.50 L - **Temperature**: 16.6°C ### Task Determine the partial pressure for each gas in mmHg and the total pressure in the flask. ### Formulae Needed: You will need the ideal gas law, which is stated as: \[ PV = nRT \] where: - \( P \) = pressure (in atm) - \( V \) = volume (in liters) - \( n \) = number of moles - \( R \) = ideal gas constant (0.0821 L·atm·K⁻¹·mol⁻¹) - \( T \) = temperature (in Kelvin) **Note:** Convert temperature to Kelvin by using \( T(K) = T(°C) + 273.15 \). ### Steps to Complete: 1. Convert the temperature from Celsius to Kelvin. 2. Calculate the moles of each gas using their respective masses and molar masses. 3. Use the ideal gas law to find the partial pressure of each gas. 4. Sum the partial pressures to find the total pressure in the flask. ### Input Fields: - CO: _______ mmHg - CO₂: _______ mmHg - SF₆: _______ mmHg - Total: _______ mmHg ### Interactive Elements: - **Buttons**: `Submit`, `Show Approach`, `Hide Tutor Steps` Make sure to fill out the pressure values in the corresponding input fields to check your results. The `Show Approach` and `Hide Tutor Steps` buttons can help you understand the method to solve this problem or hide the guiding steps if needed.
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