Thermodynamic processes are indicated in the following diagram.
Match the following:
Column I | Column II | ||
P. | Process-I | a. | Adiabatic |
Q. | Process-II | b. | Isobaric |
R. | Process-III | c. | Isochoric |
S. | Process-IV | d. | Isothermal |
1. | \(P \rightarrow \mathrm{a}, Q \rightarrow \mathrm{c}, R \rightarrow \mathrm{d}, S \rightarrow \mathrm{b}\) |
2. | \(P \rightarrow \mathrm{c}, Q \rightarrow \mathrm{a}, R \rightarrow \mathrm{d}, S \rightarrow b\) |
3. | \(P \rightarrow \mathrm{c}, Q \rightarrow \mathrm{d}, R \rightarrow \mathrm{b}, S \rightarrow a\) |
4. | \(P \rightarrow \mathrm{c}, Q \rightarrow \mathrm{d}, R \rightarrow \mathrm{b}, S \rightarrow a\) |
An ideal gas goes from state A to state B via three different processes, as indicated in the P-V diagram. If indicates the heat absorbed by the gas along the three processes and indicates the change in internal energy along the three processes respectively, then:
1. | \(\mathrm{Q}_1>\mathrm{Q}_2>\mathrm{Q}_3 \) and \(\Delta \mathrm{U}_1=\Delta \mathrm{U}_2=\Delta \mathrm{U}_3\) |
2. | \(\mathrm{Q}_3>\mathrm{Q}_2>\mathrm{Q}_1\) and \(\Delta \mathrm{U}_1=\Delta \mathrm{U}_2=\Delta \mathrm{U}_3\) |
3. | \(\mathrm{Q}_1=\mathrm{Q}_2=\mathrm{Q}_3\) and \(\Delta \mathrm{U}_1>\Delta \mathrm{U}_2>\Delta \mathrm{U}_3\) |
4. | \(\mathrm{Q}_3>\mathrm{Q}_2>\mathrm{Q}_1\) and \(\Delta \mathrm{U}_1>\Delta \mathrm{U}_2>\Delta \mathrm{U}_3\) |
In thermodynamic processes, which of the following statements is not true?
1. | In an adiabatic process, the system is insulated from the surroundings. |
2. | In an isochoric process, the pressure remains constant. |
3. | In an isothermal process, the temperature remains constant. |
4. | In an adiabatic process, \(P V^\gamma\) = constant. |
The specific heat of a gas in an isothermal process is:
1. Infinite
2. Zero
3. Negative
4. Remains constant
Two identical samples of a gas are allowed to expand, (i) isothermally and (ii) adiabatically. Work done will be:
1. | more in the isothermal process. |
2. | more in the adiabatic process. |
3. | equal in both processes. |
4. | none of the above. |
In an adiabatic expansion of a gas, if the initial and final temperatures are \(T_1\) and \(T_2\), respectively, then the change in internal energy of the gas is:
1. \(\frac{nR}{\gamma-1}(T_2-T_1)\)
2. \(\frac{nR}{\gamma-1}(T_1-T_2)\)
3. \(nR ~(T_1-T_2)\)
4. Zero
In a cyclic process, the internal energy of the gas:
1. | Increases | 2. | Decreases |
3. | Remains constant | 4. | Becomes zero |
When an ideal diatomic gas is heated at constant pressure, the fraction of the heat energy supplied which increases the internal energy of the gas is?
1. | \(2 \over 5\) | 2. | \(3 \over 5\) |
3. | \(3 \over 7\) | 4. | \(5 \over 7\) |
In the following figures, four curves A, B, C and D, are shown. The curves are:
1. | isothermal for A and D while adiabatic for B and C. |
2. | adiabatic for A and C while isothermal for B and D. |
3. | isothermal for A and B while adiabatic for C and D. |
4. | isothermal for A and C while adiabatic for B and D. |
For the indicator diagram given below, which of the following is not correct?
1. | Cycle - II is a heat engine cycle. |
2. | Net work is done on the gas in cycle I. |
3. | Work done is positive for cycle I. |
4. | Work done is positive for cycle II. |