Question
What happens to the pressure of a gas if the temperature rises? Why.
Answers
Answered by
GPT-4o mini
When the temperature of a gas increases, the pressure of that gas also tends to increase, assuming the volume remains constant. This relationship is explained by the ideal gas law, which is expressed as:
\[ PV = nRT \]
where:
- \( P \) is the pressure,
- \( V \) is the volume,
- \( n \) is the number of moles of gas,
- \( R \) is the universal gas constant,
- \( T \) is the temperature in Kelvin.
If the volume (\( V \)) and the number of moles of gas (\( n \)) are held constant, any increase in temperature (\( T \)) will lead to an increase in pressure (\( P \)). This is because, at higher temperatures, gas molecules have more kinetic energy and move more rapidly. As a result, they collide with the walls of the container more frequently and with greater force, thus increasing the pressure.
In summary, when the temperature of a gas rises, its pressure increases (at constant volume) due to the increased kinetic energy of the gas molecules leading to more frequent and forceful collisions with the container walls.
\[ PV = nRT \]
where:
- \( P \) is the pressure,
- \( V \) is the volume,
- \( n \) is the number of moles of gas,
- \( R \) is the universal gas constant,
- \( T \) is the temperature in Kelvin.
If the volume (\( V \)) and the number of moles of gas (\( n \)) are held constant, any increase in temperature (\( T \)) will lead to an increase in pressure (\( P \)). This is because, at higher temperatures, gas molecules have more kinetic energy and move more rapidly. As a result, they collide with the walls of the container more frequently and with greater force, thus increasing the pressure.
In summary, when the temperature of a gas rises, its pressure increases (at constant volume) due to the increased kinetic energy of the gas molecules leading to more frequent and forceful collisions with the container walls.