[30 pts] Consider the following scenario where three blocks are placed on top of a frictionless, weightless piston in a cylinder filled with 2 moles of an ideal gas. The surroundings are at a pressure of 1 bar. The cylinder has a radius of 0.01 meter. Block 1 has a mass of 3.2kg, Block 2 has a mass of 1.8kg, and Block 3 has a mass of 2.7kg. A. Block 1 is removed, and the system is allowed to equilibrate (achieve its equilibrium volume as determined by the Ideal Gas Law). Then Block 2 is removed, and the system is again allowed to equilibrate. Finally, Block 3 is removed, and the system is allowed to equilibrate. The entire process is performed under isothermal conditions at a temperature of 25C. i. Plot the path on a P-V diagram, using units of bar for pressure and L for volume. Label units and values. ii. Calculate the amount of work done by the gas for each step of the process and for the entire process. iii. Calculate the change in internal energy for each step of the process. iv. Calculate the amount of heat transferred at each step of the process. B. Now Consider the case where the processes occur in isothermal conditions, but the blocks are removed in reverse order (Block 3 is removed first, then Block 2, followed by Block 1). i. How does the total amount of work performed by the gas differ from Part A? ii. How do your results demonstrate the difference between path and state variables? C. Imagine a scenario where there are thousands of tiny blocks on the piston and they are removed one by one and the system allowed to equilibrate after each removal