Question

How do gas laws apply to everyday life?

Answer 1

Hint: We have to know that gas laws were the result of the study which involved the investigation of pressure, volume and temperature of the gas sample. Ideal gas features molecules which abide following rules: Ideal gas molecules do not attract or repel each other and Ideal gas molecules themselves take up no volume.

Complete answer:
We need to remember that there are three gas laws which are named as ABC’s law : Avogadro law, Boyle’s law and Charles' law. Now we will study how these laws apply to everyday life. Boyle’s law states that “In a closed system, the volume of gas is inversely proportional to the pressure exerted by the gas”. When the pressure in a closed system is doubled, the volume is reduced to half, as long as the temperature and the amount of gas are the same. Example: When a scuba diver exhales, water bubbles released grow larger as it reaches the surface. This happens since the pressure exerted by the water decreases with depth, and hence the volume of the bubbles increases as they approach the surface. Then next is Charles’s law which states that “At constant pressure, the volume of an ideal gas is directly proportional to the absolute temperature”. Example: The football which is inflated inside shrinks when taken outdoors during winter. Last is Avogadro’s Law. According to this law “At the same temperature and pressure condition, as the number of moles of gas increases the volume also increases”. Example: During the breathing process, lungs expand to fill the air while inhaling, and during the exhaling process, the volume of the lungs decreases.

Note:
We need to know that ideal gas law states that Pressure and volume is directly proportional to number of moles and temperature. The ideal gas law can be used in stoichiometry problems in which chemical reactions involve gases.