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
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![### 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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F40fff8cd-053c-4eec-9b68-327a5d917b73%2Fc1808109-a138-4021-a705-0cc48572ba71%2Fhdrucuh_processed.jpeg&w=3840&q=75)
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