A sample of hydrogen gas at a pressure of 1.09 atm and a temperature of 29.6 °C, occupies a volume of 694 mL. If the gas is compressed at constant temperature until its pressure is 1.44 atm, 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.
![### Boyles' Law Example Problem
A sample of **hydrogen gas** at a pressure of **1.09 atm** and a temperature of **29.6 °C**, occupies a volume of **694 mL**. If the gas is **compressed** at constant temperature until its pressure is **1.44 atm**, the volume of the gas sample will be \_\_\_\_\_\_ mL.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84435934-315d-4f3f-bf89-3ba66c6d068b%2Fa79132fe-7f67-4c60-9b05-6f8086b20bda%2Fkih2n6_processed.png&w=3840&q=75)
![**Example Problem for Understanding Gas Laws**
A sample of **nitrogen** gas occupies a volume of **8.00 L** at **55.0°C** and **0.920 atm**.
If it is desired to **increase** the volume of the gas sample to **9.16 L**, while **decreasing** its pressure to **0.602 atm**, the temperature of the gas sample at the new volume and pressure must be **_____°C**.
(Note: In this example problem, students would typically use the combined gas law equation to solve for the unknown temperature, \(T_2\). The combined gas law is \(\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}\), where \( P \) is pressure, \( V \) is volume, and \( T \) is temperature in Kelvins.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84435934-315d-4f3f-bf89-3ba66c6d068b%2Fa79132fe-7f67-4c60-9b05-6f8086b20bda%2Fnjkb4w_processed.png&w=3840&q=75)
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