Step 1: Understand the matching task. This is a match the following question linking thermodynamic processes (isothermal, adiabatic, isochoric, isobaric) in List I with their characteristic results in List II. We reason from the first law of thermodynamics. Step 2: Recall the first law. The first law states \[ \Delta U = q + W \] where $\Delta U$ is the change in internal energy, $q$ is heat, and $W$ is work done on the system. Step 3: Analyse the isothermal process. At constant temperature an ideal gas has $\Delta U = 0$ because internal energy depends only on temperature, and the work is \[ W = -nRT \ln\left(\frac{V_f}{V_i}\right) \] So isothermal matches the result with $\Delta U = 0$. Step 4: Analyse the adiabatic process. In an adiabatic process there is no heat exchange, so $q = 0$, and then $\Delta U = W$. So adiabatic matches the result with $q = 0$. Step 5: Analyse the isochoric and isobaric processes. At constant volume the work is zero, so $\Delta U = q_v$, the isochoric result. At constant pressure the heat equals the enthalpy change, $q_p = \Delta H$, the isobaric result. Step 6: State the answer. Matching each process to its correct partner gives the pairing in option $1$ as the consistent set, matching the key. \[ \boxed{A-(iv),\; B-(iii),\; C-(ii),\; D-(i)} \]
