we have a cylinder which has a capacity of 12 atm at . now if we reduce the pressure to a low value like 3 atm, at 300k . if the temperature is more than 1200k ,the cylinder will explode.we found yhis value using gay lussac's law. but here in today's class we learnt that the KE of gases produces thermal energy. if the pressure of the gas is less how can so much heat get produced? is this example violating the kinetic molecular theory of gases?
Dear Sukanya Roy,
In lussac law P=kT
so P1/T1=P2/T2 and P2 will be 12 atm at 1200K
If you increase the T more than 1200K the pressure will exceed 12atm and cyclinder will explode.
On the other hand K.E.=3/2 kT here k is boltzmann costant
so we can say K.E.. of molecules(gas) are directly proportional to T hence when we increase the T the movement of gas particle will be more
and hence exerted P will be more. (due to more collision with wall)
Both are different phenomenon but the effect of T is more than P or V as far as K.E. is concern.
Regards
In lussac law P=kT
so P1/T1=P2/T2 and P2 will be 12 atm at 1200K
If you increase the T more than 1200K the pressure will exceed 12atm and cyclinder will explode.
On the other hand K.E.=3/2 kT here k is boltzmann costant
so we can say K.E.. of molecules(gas) are directly proportional to T hence when we increase the T the movement of gas particle will be more
and hence exerted P will be more. (due to more collision with wall)
Both are different phenomenon but the effect of T is more than P or V as far as K.E. is concern.
Regards