A sample of helium gas at a pressure of 727 torr and a temperature of 23.8°C, occupies a volume of 435 mL. If the gas is allowed to expand at constant temperature until its pressure is 424 torr, the volume of the gas sample will be mL.
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.
![### Exploring Gas Laws: Volume and Pressure Relationship
**Use the References** to access important values if needed for this question.
A sample of **helium** gas at a pressure of **727 torr** and a temperature of **23.8°C** occupies a volume of **435 mL**. If the gas is allowed to expand at constant temperature until its pressure is **424 torr**, the volume of the gas sample will be ______ mL.
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This exercise involves the application of Boyle's Law, which states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with its pressure. Mathematically, this relationship is expressed as:
\[ P_1 V_1 = P_2 V_2 \]
Where:
- \( P_1 \) and \( V_1 \) are the initial pressure and volume of the gas.
- \( P_2 \) and \( V_2 \) are the final pressure and volume of the gas.
By understanding and manipulating these variables, we can predict how a gas will behave under different conditions of pressure while maintaining its temperature. This exercise also underscores the importance of keeping the units consistent when performing calculations.
For additional assistance and review on this topic, use the blue "Review Topics" or "References" links provided on your educational platform.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9ee6479a-9360-421e-a0d3-69e759864a42%2F4844e5dd-27f3-431a-ab59-07ed91a98a24%2Flcgnhzf.jpeg&w=3840&q=75)
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