To determine in which process heat is neither absorbed nor released, we need to understand the characteristics of each thermodynamic process:$\\$• Isothermal Process:$\\$In an isothermal process, the temperature of the system remains constant.$\\$According to the first law of thermodynamics, $\Delta U = Q - W,$ where $\Delta U$ is the change in internal energy,$\\ Q$ is the heat exchanged, and $W$ is the work done by the system.$\\$For an ideal gas, if the temperature is constant, $\Delta U = 0,$ so $Q = W. \\$Thus, heat is exchanged in an isothermal process.$\\$• Adiabatic Process:$\\$In an adiabatic process, no heat is exchanged with the surroundings,$\\$which means $Q = 0. \\$Therefore, the change in internal energy is equal to the work done on or by the system: $\Delta U = -W. \\$This is the process where heat is neither absorbed nor released.$\\$• Isobaric Process:$\\$In an isobaric process, the pressure remains constant.$\\$Heat can be absorbed or released to maintain constant pressure, so $Q \neq 0. \\$• Isochoric Process:$\\$In an isochoric process, the volume remains constant.$\\$No work is done ($W = 0$), but heat can be absorbed or released to change the internal energy,$\\$so $Q = \Delta U. \\$Therefore, the correct answer is the adiabatic process, where heat is neither absorbed nor released.$\\$This corresponds to Option 2.