The ideal gas equation is;
Pressure* volume = number of moles*ideal gas constant* temperature
PV = nRT
If the number of moles and pressure of the gas are kept constant, then volume of the gas increases with increase in temperature.
The relation between kinetic energy and temperature is;
Kinetic energy = 3/2 k T
'k' is a constant. The above relation shows that the kinetic energy of the gas or air molecules increases with increase in temperature.
The kinetic energy of particles is equal to the half of mass times square of mean velocity. So;
Average kinetic energy = 1/2 m (mean velocity of molecules )2
OR
3/2 kT = 1/2 m (mean square velocity)
Vrms = [3k T]1/2
'rms' denotes root mean square velocity of particles. The relation between velocity and temperature shows that both velocity and temperature are directly proportional to each other.
Pressure* volume = number of moles*ideal gas constant* temperature
PV = nRT
If the number of moles and pressure of the gas are kept constant, then volume of the gas increases with increase in temperature.
The relation between kinetic energy and temperature is;
Kinetic energy = 3/2 k T
'k' is a constant. The above relation shows that the kinetic energy of the gas or air molecules increases with increase in temperature.
The kinetic energy of particles is equal to the half of mass times square of mean velocity. So;
Average kinetic energy = 1/2 m (mean velocity of molecules )2
OR
3/2 kT = 1/2 m (mean square velocity)
Vrms = [3k T]1/2
'rms' denotes root mean square velocity of particles. The relation between velocity and temperature shows that both velocity and temperature are directly proportional to each other.
