In an isothermal process system is in contact with outside heat reservior and the change occur slowly so as to facilitate to adjust temp and in adiabatic process system is isolated. Then my question is even if adiabatic system is isolated then how the temperature changes.
In an isothermal process system is in contact with outside heat reservior and the change occur slowly so as to facilitate to adjust temp and in adiabatic process system is isolated. Then my question is even if adiabatic system is isolated then how the temperature changes.
Remember adiabatic process implies process in which no heat exchange takes place between the system and the surrounding i.e. neither heat is supplied nor heat is loosed.
Temperature of gases changes only when internal energy of the gases changes.
Net heat of the system constant means dq = 0
dq= du+dw, to maintain dq = 0, you can have many possible set of values of du and dw. Like whatever amount work you do, say dw, to maintain addition of du and dw always as zero, du = -dw. So any amount of work you do , du becomes negative of that work you perform to maintain net heat of the system as constant (i.e. dq as zero). So even while maintaining addition of du and dw as zero, you can have infinite possible values of du and dw ( i.e. do any aribitary work and du becomes the negative of the work you performed and hence addition becomes always zero)
Temperature of the gas is related to du by du = nCvΔT. Hence for all those infinite possible values of du, you will have infinite possible temperatures, still maintaining constant net heat of the system .i.e dq as zero.
So in an adiabatic process, if you performed work, then du has to change to a value which is negative of the amount of work you performed (otherwise you won't be able to maintain their addition to be zero) , and as du has to change, hence temperature also changes.
So every time you perform work in an adiabatic container, temperature has to change.
Remember adiabatic process implies process in which no heat exchange takes place between the system and the surrounding i.e. neither heat is supplied nor heat is loosed.
Temperature of gases changes only when internal energy of the gases changes.
Net heat of the system constant means dq = 0
dq= du+dw, to maintain dq = 0, you can have many possible set of values of du and dw. Like whatever amount work you do, say dw, to maintain addition of du and dw always as zero, du = -dw. So any amount of work you do , du becomes negative of that work you perform to maintain net heat of the system as constant (i.e. dq as zero). So even while maintaining addition of du and dw as zero, you can have infinite possible values of du and dw ( i.e. do any aribitary work and du becomes the negative of the work you performed and hence addition becomes always zero)
Temperature of the gas is related to du by du = nCvΔT. Hence for all those infinite possible values of du, you will have infinite possible temperatures, still maintaining constant net heat of the system .i.e dq as zero.
So in an adiabatic process, if you performed work, then du has to change to a value which is negative of the amount of work you performed (otherwise you won't be able to maintain their addition to be zero) , and as du has to change, hence temperature also changes.
So every time you perform work in an adiabatic container, temperature has to change.
