A closed system of gas is taken from an initial equilibrium state A to a final equilibrium state C in two distinct steps described below.
Step 1 (A→B): The gas is compressed adiabatically so that the surroundings do 1.50×103J of work on the gas.
Step 2 (B→C): Keeping the volume constant, the gas is now supplied with 1.20×103J of heat from a hot reservoir.
No other forms of energy transfer occur.
(i) For each step, calculate the change in internal energy of the system, clearly stating the sign of the change.
(ii) Determine the net work done by the system in the entire A→C transformation.
(iii) Compute the overall change in internal energy between states A and C.
(iv) Show numerically that the First Law of Thermodynamics is satisfied for the complete A→C path.