Q. No.The volume \((V)\) of a monatomic gas varies with its temperature \((T),\) as shown in the graph. The ratio of work done by the gas to the heat absorbed by it when it undergoes a change from state \(A\) to state \(B\) will be:
1.
\(\dfrac{2}{5}\)
2.
\(\dfrac{2}{3}\)
3.
\(\dfrac{1}{3}\)
4.
\(\dfrac{2}{7}\)
| 1. | \(26.8\%\) | 2. | \(20\%\) |
| 3. | \(6.25\%\) | 4. | \(12.5\%\) |
A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is again reduced to half. Then,
| 1. | compressing the gas through an adiabatic process will require more work to be done. |
| 2. | compressing the gas isothermally or adiabatically will require the same amount of work. |
| 3. | which of the case (whether compression through isothermal or through the adiabatic process) requires more work will depend upon the atomicity of the gas. |
| 4. | compressing the gas isothermally will require more work to be done. |
An ideal gas is compressed to half its initial volume using several processes. Which of the processes results in the maximum work done on the gas?
1. adiabatic
2. isobaric
3. isochoric
4. isothermal
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. | \(64P\) | 2. | \(32P\) |
| 3. | \(\frac{P}{64}\) | 4. | \(16P\) |
A thermodynamic system undergoes a cyclic process \(ABCDA\) as shown in Fig. The work done by the system in the cycle is:
| 1. | \( P_0 V_0 \) | 2. | \( 2 P_0 V_0 \) |
| 3. | \(\dfrac{P_0 V_0}{2} \) | 4. | zero |
| 1. | \(1000~\text{J}\) | 2. | zero |
| 3. | \(-2000~\text{J}\) | 4. | \(2000~\text{J}\) |
| 1. | \(\dfrac{R}{\gamma -1}\) | 2. | \(\dfrac{\gamma -1}{R}\) |
| 3. | \(\gamma R \) | 4. | \(\dfrac{\left ( \gamma -1 \right )R}{\left ( \gamma +1 \right )}\) |
1. \(2\)
2. \(5/3\)
3. \(3/2\)
4. \(4/3\)
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