A mixture of 0.220 moles CO, 0.350 moles F2 and 0.640 moles Ne has a total pressure of 2.95 atm. What is the partial pressure of CO? 0.649 atm 0.955 atm 0.536 atm 1.54 atm 1.86 atm O
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.
![### Partial Pressure Calculation in Gas Mixtures
**Problem Statement:**
A mixture of 0.220 moles CO, 0.350 moles F₂, and 0.640 moles Ne has a total pressure of 2.95 atm. What is the partial pressure of CO?
**Multiple Choice Answers:**
- 0.649 atm
- 0.955 atm
- 0.536 atm
- 1.54 atm
- 1.86 atm
### Explanation:
To determine the partial pressure of CO in the mixture, one can utilize Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas in the mixture. The partial pressure of each gas is calculated as follows:
\[ P_i = \chi_i \times P_{\text{total}} \]
where:
- \( P_i \) is the partial pressure of the gas,
- \( \chi_i \) is the mole fraction of the gas,
- \( P_{\text{total}} \) is the total pressure of the mixture.
First, calculate the total moles of the gas mixture:
\[ \text{Total moles} = 0.220 + 0.350 + 0.640 = 1.21 \text{ moles} \]
Next, calculate the mole fraction of CO:
\[ \chi_{\text{CO}} = \frac{0.220}{1.21} \approx 0.182 \]
Finally, use the mole fraction to find the partial pressure of CO:
\[ P_{\text{CO}} = 0.182 \times 2.95 \approx 0.537 \text{ atm} \]
Thus, the partial pressure of CO is closest to:
\[ \boxed{0.536 \text{ atm}} \]
### Conclusion:
The partial pressure of CO in the given gas mixture is \(0.536 \) atm. The correct answer from the given choices is therefore 0.536 atm.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10c6e2dc-d615-4613-bf12-6e31522fc631%2Fa98d0859-455c-4eba-a67d-c99bc17ab9ee%2Fmrw6628_processed.jpeg&w=3840&q=75)
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