Question

Work done in expansion of ideal gas

Answer 1

Answer:

An isothermal process is a change of a system, in which the temperature remains constant: ΔT =0. This typically occurs when a system is in contact with an outside thermal reservoir (heat bath), and the change in the system will occur slowly enough to allow the system to continue to adjust to the temperature of the reservoir through heat exchange. In contrast, an adiabatic process is where a system exchanges no heat with its surroundings (Q = 0). In other words, in an isothermal process, the value ΔT = 0 and therefore the change in internal energy ΔU = 0 (only for an ideal gas) but Q ≠ 0, while in an adiabatic process, ΔT ≠ 0 but Q = 0.

Simply, we can say that in isothermal processes

{\displaystyle T={\text{constant}}} {\displaystyle T={\text{constant}}}

{\displaystyle \Delta T=0} {\displaystyle \Delta T=0}

{\displaystyle dT=0} {\displaystyle dT=0}

while in adiabatic processes

{\displaystyle Q=0.} {\displaystyle Q=0.}