A gas mixture containing oxygen, nitrogen, and helium exerts a total pressure of 925 torr. If the partial pressures are oxygen 425 torr and helium 75 torr, what is the partial pressure, in torr, of the nitrogen in the mixture? Partial pressure of nitrogen in the mixture = torr?
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.
A gas mixture containing oxygen, nitrogen, and helium exerts a total pressure of 925 torr. If the
partial pressures are oxygen 425 torr and helium 75 torr, what is the partial pressure, in torr, of the
nitrogen in the mixture?
Partial pressure of nitrogen in the mixture =
torr?
![**Question:**
A gas mixture containing oxygen, nitrogen, and helium exerts a total pressure of 925 torr. If the partial pressures are oxygen 425 torr and helium 75 torr, what is the partial pressure, in torr, of the nitrogen in the mixture?
**Solution:**
Partial pressure of nitrogen in the mixture = _________ torr?
**Methodology:**
To find the partial pressure of nitrogen, we will use Dalton's Law of Partial Pressures, which states that the total pressure of a mixture of gases is the sum of the partial pressures of each individual gas:
\[ P_{\text{total}} = P_{\text{oxygen}} + P_{\text{helium}} + P_{\text{nitrogen}} \]
Given:
- Total pressure (\(P_{\text{total}}\)) = 925 torr
- Partial pressure of oxygen (\(P_{\text{oxygen}}\)) = 425 torr
- Partial pressure of helium (\(P_{\text{helium}}\)) = 75 torr
The partial pressure of nitrogen (\(P_{\text{nitrogen}}\)) can be calculated by rearranging the formula:
\[ P_{\text{nitrogen}} = P_{\text{total}} - (P_{\text{oxygen}} + P_{\text{helium}}) \]
\[ P_{\text{nitrogen}} = 925 \, \text{torr} - (425 \, \text{torr} + 75 \, \text{torr}) \]
\[ P_{\text{nitrogen}} = 925 \, \text{torr} - 500 \, \text{torr} \]
\[ P_{\text{nitrogen}} = 425 \, \text{torr} \]
**Conclusion:**
The partial pressure of nitrogen in the mixture is 425 torr.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdd69b61d-2b24-47af-96a9-508df8b58224%2Fd3c33206-9268-4e82-af49-e777357d86cc%2Fiaxj2zc_processed.jpeg&w=3840&q=75)
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