The figure below shows two paths that may be taken by gas to go from state \(A\) to state \(C\).
In process \(AB\), \(400~\text{J}\) of heat is added to the system, and in process \(BC\), \(100~\text{J}\) of heat is added to the system. The heat absorbed by the system in the process \(AC\) will be:
1. \(380~\text{J}\)
2. \(500~\text{J}\)
3. \(460~\text{J}\)
4. \(300~\text{J}\)
1. | \(10~\text{J}\) | 2. | \(12~\text{J}\) |
3. | \(36~\text{J}\) | 4. | \(6~\text{J}\) |
An ideal gas goes from state \(A\) to state \(B\) via three different processes as indicated in the \((P\text-V)\) diagram.
If \(Q_1,Q_2,Q_3\) indicate the heat absorbed by the gas along the three processes and \(\Delta U_1, \Delta U_2, \Delta U_3\) indicate the change in internal energy along the three processes respectively, then:
1. | \(Q_3>Q_2>Q_1\) and \(\Delta U_1= \Delta U_2= \Delta U_3\) |
2. | \(Q_1=Q_2=Q_3\) and \(\Delta U_1> \Delta U_2> \Delta U_3\) |
3. | \(Q_3>Q_2>Q_1\) and \(\Delta U_1> \Delta U_2> \Delta U_3\) |
4. | \(Q_1>Q_2>Q_3\) and \(\Delta U_1= \Delta U_2= \Delta U_3\) |
During an isothermal expansion, a confined ideal gas does -150 J of work against its surrounding. This implies that:
1. | 300 J of heat has been added to the gas. |
2. | no heat is transferred because the process is isothermal. |
3. | 150 J of heat has been added to the gas. |
4. | 150 J of heat has been removed from the gas. |
If \(\Delta U\) and \(\Delta W\) represent the increase in internal energy and work done by the system respectively in a thermodynamical process, which of the following is true?
1. | \(\Delta U=-\Delta W\), in an adiabatic process |
2. | \(\Delta U=\Delta W\) , in an isothermal process |
3. | \(\Delta U=\Delta W\), in an adiabatic process |
4. | \(\Delta U=-\Delta W\), in an isothermal process |
The internal energy change in a system that has absorbed \(2\) kcal of heat and done \(500\) J of work is:
1. \(8900\) J
2. \(6400\) J
3. \(5400\) J
4. \(7900\) J