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.
![### Determining the Pressure of a Gas in a Manometer
#### Problem Statement:
If the atmospheric pressure is at 780 mmHg, what is the pressure of the gas in the manometer?
#### Diagram Description:
In the provided diagram, a manometer is illustrated along with a container holding gas. The manometer is a U-shaped tube filled with mercury (Hg). Here are specific details from the diagram:
- **Left Side:** Connected to the gas container labeled "gas."
- **Right Side:** Open to the atmosphere, marked "atmosphere" with an arrow pointing towards the opening.
- **Mercury (Hg) Levels:** The mercury levels on both sides of the manometer are not equal. The left side is lower while the right side, which is exposed to the atmospheric pressure, is higher.
- **Height Difference:** The height difference between the mercury levels on both sides is marked as 14.7 cm.
#### Calculation Details:
To determine the pressure of the gas in the manometer:
1. **Convert the Height Difference to mmHg:**
- Given height difference: 14.7 cm
- Conversion: 14.7 cm Hg * 10 mm/cm = 147 mmHg
(Note: 1 cm Hg = 10 mm Hg)
2. **Calculate the Gas Pressure:**
- Since the mercury in the manometer on the side open to the atmosphere is higher, it indicates that the gas pressure is greater than the atmospheric pressure.
- Formula used:
\[
\text{Pressure of Gas} = \text{Atmospheric Pressure} + \text{Difference in Mercury Levels}
\]
- Substitute the given values:
\[
\text{Pressure of Gas} = 780 \text{ mmHg} + 147 \text{ mmHg}
\]
\[
\text{Pressure of Gas} = 927 \text{ mmHg}
\]
#### Conclusion:
The pressure of the gas in the manometer is **927 mmHg**.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbe190d63-587e-4b92-bb0f-2dc0c233d9b9%2Fccb6918d-35ea-487a-84af-cb46aca46dcc%2Fpzvjz9i_processed.png&w=3840&q=75)
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