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abcd8989
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Why it is not necessary for an ideal gas to obey Charles's law, but Boyle's only?
An ideal gas obeys the ideal gas law. What makes you think that Boyles' law (which says that P varies inversely as V - temperature being constant) or Charles' law (which, it appears to me, simply says that V is proportional to temperature at constant pressure) are not obeyed by an ideal gas?abcd8989 said:Why it is not necessary for an ideal gas to obey Charles's law, but Boyle's only?
Charles's Law states that at a constant pressure, the volume of an ideal gas is directly proportional to its absolute temperature. Boyle's Law states that at a constant temperature, the volume of an ideal gas is inversely proportional to its pressure.
Both laws describe the relationship between volume and either temperature or pressure of an ideal gas. They are also both based on the concept of the ideal gas, which assumes that the gas particles have no volume and do not interact with each other.
Charles's Law can be expressed as V1/T1 = V2/T2, where V is the volume and T is the absolute temperature. Boyle's Law can be expressed as P1V1 = P2V2, where P is the pressure and V is the volume.
Real gases do not always behave like ideal gases, so the relationship described by these laws may not always hold true. However, at moderate temperatures and pressures, real gases can often approximate ideal gases, and the laws can still be used as a guide.
These laws are commonly used in chemistry and physics to predict the behavior of gases in various situations. For example, they can be used to calculate the volume of a gas at a given temperature and pressure, or to determine the pressure required to compress a gas to a certain volume. They are also used in industries such as engineering and meteorology to understand the behavior of gases in different environments.