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
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
- [NEET 2016]
- A
Compressing the gas through adiabatic process will require more work to be done.
- B
Compressing the gas isothermally or adiabatically will require the same amount of work.
- C
Which of the case (whether compression through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.
- D
Compressing the gas isothermally will require more work to be done.
Similar Questions
In Column$-I$ process and in Column$-II$ first law of thermodynamics are given. Match them appropriately :
Column$-I$
Column$-II$
$(a)$ Adiabatic
$(i)$ $\Delta Q = \Delta U$
$(b)$ Isothermal
$(ii)$ $\Delta Q = \Delta W$
$(iii)$ $\Delta U = -\Delta W$
In Column$-I$ process and in Column$-II$ first law of thermodynamics are given. Match them appropriately :
| Column$-I$ | Column$-II$ |
| $(a)$ Adiabatic | $(i)$ $\Delta Q = \Delta U$ |
| $(b)$ Isothermal | $(ii)$ $\Delta Q = \Delta W$ |
| $(iii)$ $\Delta U = -\Delta W$ |
In the following $P-V$ diagram two adiabatics cut two isothermals at temperatures $T_1$ and $T_2$ (fig.). The value of $\frac{{{V_a}}}{{{V_d}}}$ will be
In the following $P-V$ diagram two adiabatics cut two isothermals at temperatures $T_1$ and $T_2$ (fig.). The value of $\frac{{{V_a}}}{{{V_d}}}$ will be
Consider that an ideal gas ($n$ moles) is expanding in a process given by $P = f (V)$, which passes through a point $(V_0, \,p_0)$. Show that the gas is absorbing heat at $(p_0,\, V_0)$ if the slope of the curve $P = f (V)$ is larger than the slope of the adiabatic passing through $(p_0,\, V_0)$.
Consider that an ideal gas ($n$ moles) is expanding in a process given by $P = f (V)$, which passes through a point $(V_0, \,p_0)$. Show that the gas is absorbing heat at $(p_0,\, V_0)$ if the slope of the curve $P = f (V)$ is larger than the slope of the adiabatic passing through $(p_0,\, V_0)$.
$Assertion :$ Adiabatic expansion is always accompanied by fall in temperature.
$Reason :$ In adiabatic process, volume is inversely proportional to temperature.
$Assertion :$ Adiabatic expansion is always accompanied by fall in temperature.
$Reason :$ In adiabatic process, volume is inversely proportional to temperature.
- [AIIMS 2011]
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 during these processes in the random order.:
Column $I$
Column $II$
$(p)$ isobaric
$(x)$ $\frac{{PV(1 - {2^{1 - \gamma }})}}{{\gamma - 1}}$
$(q)$ isothermal
$(y)$ $PV$
$(r)$ adiabatic
(z) $PV\,\iota n\,2$
The correct matching of column $I$ and column $II$ is given by
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 during these processes in the random order.:
| Column $I$ | Column $II$ |
| $(p)$ isobaric | $(x)$ $\frac{{PV(1 - {2^{1 - \gamma }})}}{{\gamma - 1}}$ |
| $(q)$ isothermal | $(y)$ $PV$ |
| $(r)$ adiabatic | (z) $PV\,\iota n\,2$ |
The correct matching of column $I$ and column $II$ is given by