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Apex
Charle's law describes the relationship between temperature and volume of a gas at a fixed pressure. The relationship is (T/V)=k. k is a constant. Therefore, T1/V1=T2/V2. So if you decrease the volume of the gas, you must also decrease the temperature in order to maintain the fixed pressure.
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The molecules will not collide as often with the walls decreasing the volume
Answer: No, this is not according to Charles law; however according to Boyles law this statement is correct ('true').Charles' law states: When the pressure on a sample of a gas is held constant, the Kelvin temperature and the volume will be directly related.Boyle's law describes how the pressure of a gas tends to decrease as the volume of a gas increases when temperature is held constant.
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as the pressure decreases the volume of gas increases at constant temperature
Charles's law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its absolute temperature. For fixed mass of an Ideal Gas at constant pressure the volume it occupies is directly proportional to its absolute temperature. So, if you double the absolute temperature of a gas while holding its pressure constant, the volume has to double. There is no such thing as an Ideal Gas. So, doubling the temperature of a real gas will not exactly double its volume. However, the general principle hold true. If you increase the temperature of any gas at constant pressure the volume it occupies will increase.
According to Charles's Law, temperature and volume are proportional; that is, as temperature increases, volume increases by the same factor, and vice versa. Thus, as the temperature of the air inside the beach ball decreases, its volume decreases as well.
According to Charles law, the volume of gas decreases with lower temperatures and increases with higher temperatures
Charles's Law
Charles found that when the temperature of a gas is increased at constant pressure, its volume increases. When the temperature of a gas is decreased at constant pressure, its volume decreases.
As indicated by Charles's Law, at constant pressure, the volume decreases when the temperature decreases. This is due to slowed collisions between molecules.
The molecules will not collide as often with the walls decreasing the volume
Charles' Law says that as pressure on a gas decreases, its volume increases. Charles' Law is an example of an inverse relationship.t It is not Charle's law It is Boyle's law Charles law states at constant volume, pressure is proportional to kelvin temperature And at constant pressure volume is proportional to kelvin temperature But Boyle's law states that at constant temperature pressure is inversely related to volume
Charles' Law says that as pressure on a gas decreases, its volume increases. Charles' Law is an example of an inverse relationship.t It is not Charle's law It is Boyle's law Charles law states at constant volume, pressure is proportional to kelvin temperature And at constant pressure volume is proportional to kelvin temperature But Boyle's law states that at constant temperature pressure is inversely related to volume
Answer: No, this is not according to Charles law; however according to Boyles law this statement is correct ('true').Charles' law states: When the pressure on a sample of a gas is held constant, the Kelvin temperature and the volume will be directly related.Boyle's law describes how the pressure of a gas tends to decrease as the volume of a gas increases when temperature is held constant.
According the kinetic theory of gases and Charles law increasing the temperature of a gas increases its volume. This is due to the increased collisions between gas molecules. With a larger volume and the same mass the gas's density decreases.
decreases
== == According to Charles's Law, "At constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature (in Kelvin) increases or decreases." Therefore, if the temperature of the gas is decreased, the volume of the gas will decrease proportionally, and the balloon will contract.