Refer to figure given below. Let \(ΔU_1\) and \(ΔU_2\) be the change in internal energy in processes \(A\) and \(B\) respectively, \(ΔQ\) be the net heat given to the system in process \(A + B\) and \(ΔW\) be the net work done by the system in the process \( A + B.\)

     
For the above figure:

(a)	\(\Delta U_1+\Delta U_2=0\)
(b)	\(\Delta U_1-\Delta U_2=0\)
(c)	\(\Delta Q-\Delta W=0\)
(d)	\(\Delta Q+\Delta W=0\)

Choose the correct option:
1. (a), (b) 
2. (b), (c) 
3. (c), (d) 
4. (a), (c) 

The internal energy of an ideal gas decreases by the same amount as the work done by the system. Then:

Choose the correct option from the given ones:  

The work done by a sample of an ideal gas in the process \(A\) is doubles the work done in another process \(B.\) The temperature rises through the same amount in the two processes. If \(C_A\) and \(C_B\) are the molar heat capacities for the two processes, then:
1. \(C_A = C_B\)
2. \(C_A <C_B\)
3. \(C_A >C_B\)
4. \(C_A\) and \(C_B\) cannot be defined

For a solid with a small expansion coefficient is:
1. \(C_P - C_V = R\)
2. \(C_P= C_V \)
3. \(C_P\) is slightly greater than \(C_V\)
4. \(C_P\) is slightly less than \(C_V\)

The value of C_p – C_V is 1.00 R for a gas sample in state A and is 1.08 R in state B. Let p_A , p_B denote the pressures and T_A and T_B denote the temperatures of the states A and B respectively. Most likely

1.  p_A < p_B and T_A > T_B

2.  p_A > p_B and T_A < T_B 

3.  p_A = P_B and T_A < T_B

4.  p_A > p_B and T_A = T_B

The figure shows a process on a gas in which pressure and volume both change. The molar heat capacity for this process is \(C\). Then;

1. \(C = 0\)

2. \(C = C_V\)

3. \(C>C_V\)

4. \(C<C_V\)

The molar heat capacity for the process shown in the following figure is:
     
1.  \(C = C_P\)

2.  \(C = C_V\)

3.  \(C > C_V\)

4.  \(C =0\)

In an isothermal process on an ideal gas, the pressure increases by \(0.5\%.\) The volume decreases by about:
1. \(0.25\%\)
2. \(0.5\%\)
3. \(0.7\%\)
4. \(1\%\)