Match List-$I$ with List-$II$:
List-$I$ List-$II$ $(a)$ Isothermal $(i)$ Pressure constant $(b)$ Isochoric $(ii)$ Temperature constant $(c)$ Adiabatic $(iii)$ Volume constant $(d)$ Isobaric $(iv)$ Heat content is constant
Choose the correct answer from the options given below:
| List-$I$ | List-$II$ |
|---|---|
| $(a)$ Isothermal | $(i)$ Pressure constant |
| $(b)$ Isochoric | $(ii)$ Temperature constant |
| $(c)$ Adiabatic | $(iii)$ Volume constant |
| $(d)$ Isobaric | $(iv)$ Heat content is constant |
Choose the correct answer from the options given below:
- A$(a) \rightarrow (i), (b) \rightarrow (iii), (c) \rightarrow (ii), (d) \rightarrow (iv)$
- B$(a) \rightarrow (ii), (b) \rightarrow (iii), (c) \rightarrow (iv), (d) \rightarrow (i)$
- C$(a) \rightarrow (ii), (b) \rightarrow (iv), (c) \rightarrow (iii), (d) \rightarrow (i)$
- D$(a) \rightarrow (iii), (b) \rightarrow (ii), (c) \rightarrow (i), (d) \rightarrow (iv)$
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Similar Questions
An ideal gas at pressure $P$ and volume $V$ is expanded to volume $2V$. Column $I$ represents the thermodynamic processes used during expansion. Column $II$ represents the work done during these processes in random order:
Column $I$ Column $II$ $(p)$ isobaric $(x)$ $\frac{PV(1 - 2^{1 - \gamma})}{\gamma - 1}$ $(q)$ isothermal $(y)$ $PV$ $(r)$ adiabatic $(z)$ $PV \ln 2$
The correct matching of column $I$ and column $II$ is given by:
| Column $I$ | Column $II$ |
| $(p)$ isobaric | $(x)$ $\frac{PV(1 - 2^{1 - \gamma})}{\gamma - 1}$ |
| $(q)$ isothermal | $(y)$ $PV$ |
| $(r)$ adiabatic | $(z)$ $PV \ln 2$ |
The correct matching of column $I$ and column $II$ is given by:
Difficult
View Solution$A$ reversible cyclic process for an ideal gas is shown below. Here,$P, V$,and $T$ are pressure,volume,and temperature,respectively. The thermodynamic parameters $q, w, H$,and $U$ are heat,work,enthalpy,and internal energy,respectively.
The correct option$(s)$ is (are):
$(A)$ $q_{AC} = \Delta U_{BC}$ and $W_{AB} = P_2(V_2 - V_1)$
$(B)$ $W_{BC} = P_2(V_2 - V_1)$ and $q_{BC} = H_{AC}$
$(C)$ $\Delta H_{CA} < \Delta U_{CA}$ and $q_{AC} = \Delta U_{BC}$
$(D)$ $q_{BC} = \Delta H_{AC}$ and $\Delta H_{CA} > \Delta U_{CA}$
The correct option$(s)$ is (are):
$(A)$ $q_{AC} = \Delta U_{BC}$ and $W_{AB} = P_2(V_2 - V_1)$
$(B)$ $W_{BC} = P_2(V_2 - V_1)$ and $q_{BC} = H_{AC}$
$(C)$ $\Delta H_{CA} < \Delta U_{CA}$ and $q_{AC} = \Delta U_{BC}$
$(D)$ $q_{BC} = \Delta H_{AC}$ and $\Delta H_{CA} > \Delta U_{CA}$
One gram of a liquid is converted to vapour at $3 \times 10^5 \text{ Pa}$ pressure. If $10\%$ of the heat supplied is used for increasing the volume by $1600 \text{ cm}^3$ during this phase change, then the increase in internal energy in the process will be
DifficultMHT CET 2026
View SolutionNeon gas of a given mass expands isothermally to double its volume. What should be the further fractional decrease in pressure,so that the gas when adiabatically compressed from that state,reaches the original state?
Medium
View SolutionAn ideal gas undergoes a cyclic process through various thermodynamic states. The heat energy $(Q)$ and work $(W)$ associated with these states are given as follows:
$Q_1 = 6000 \ J, Q_2 = -5500 \ J, Q_3 = -3300 \ J, Q_4 = 3500 \ J,$
$W_1 = 2500 \ J, W_2 = -1000 \ J, W_3 = -1200 \ J, W_4 = x \ J$
If the ratio of the net work done to the net heat absorbed is $\eta$, then the values of $x$ and $\eta$ are respectively:
$Q_1 = 6000 \ J, Q_2 = -5500 \ J, Q_3 = -3300 \ J, Q_4 = 3500 \ J,$
$W_1 = 2500 \ J, W_2 = -1000 \ J, W_3 = -1200 \ J, W_4 = x \ J$
If the ratio of the net work done to the net heat absorbed is $\eta$, then the values of $x$ and $\eta$ are respectively:
Difficult
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