Final answer:
The question requires the calculation of parameters for an isobaric process and an isochoric process using given values and thermodynamic laws. Work can be calculated for the isobaric process and it's understood that no work is done in the isochoric process due to constant volume.
Step-by-step explanation:
The question involves determining the values for various parameters in different thermodynamic processes. We have an isobaric process, where pressure (P) is constant, and an isochoric process, where volume (V) is constant.
For Process A (Isobaric process): The values given are P = 2 atm, V1 = 2 L, V2 = 4 L, and n = 1 mole. Using the ideal gas law PV = nRT, we can find parameters like the change in temperature. However, since the pressure is constant, the work done on the gas can be calculated using W = P(V2 - V1).
For Process B (Isochoric process): The values given are V = 2 L, P1 = 2 atm, P2 = 4 atm, and N1 = 1 mole. Since the volume is constant, there is no work done during this process (work, in a thermodynamic sense, is related to volume change). The change in internal energy can be found using the first law of thermodynamics, ΔU = Q - W, where ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done by the system.