Consider the following two statements.

The figure shows the (P-V) diagram of an ideal gas undergoing a change of state from A to B. Four different paths I, II, III and IV, as shown in the figure, may lead to the same change of state.
               

Which of the following options contains only correct statements?

A gas expands from \(\mathrm{i}\) to \(\mathrm{f}\) along the three paths indicated. The work done along the three paths denoted by ${\mathrm{W}}_1, {\mathrm{W}}_2, \mathrm{and} {\mathrm{W}}_3$ have the relationship:
                
1.  ${\mathrm{W}}_1 < {\mathrm{W}}_2< {\mathrm{W}}_3$

2.  ${\mathrm{W}}_2 < {\mathrm{W}}_1 = {\mathrm{W}}_3$

3.  ${\mathrm{W}}_2 < {\mathrm{W}}_1 < {\mathrm{W}}_3$

4.  ${\mathrm{W}}_1 > {\mathrm{W}}_2 > {\mathrm{W}}_3$

An ideal gas is made to undergo a cycle depicted by the \((P-V)\) diagram alongside. If the curved line from \(A\) to \(B\) is adiabatic, then:
                    

In this \((P-V)\) diagram below the dashed curved line is adiabatic.

                       
For a process, that is described by a straight line joining two points \(X\) and \(Y\) on the adiabat (solid line In the diagram) heat is:
(Consider the variations in temperature from \(X\) to \(Y\) along the straight line.)

An ideal gas is taken reversibly around the cycle a-b-c-d-a as shown on the \(T\) (temperature) -\(S\) (entropy) diagram.
                
The most appropriate representation of the above cycle on a \(U\) (internal energy) -\(V\) (volume) diagram is:

1.		2.
3.		4.