(A) Let the initial volume be $V_1 = V$ and the final volume be $V_2 = V/2$.In a $P-V$ diagram,the work done during a compression process is represent

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Compressing the gas through adiabatic process will require more work to be done.

(A) Let the initial volume be $V_1 = V$ and the final volume be $V_2 = V/2$.In a $P-V$ diagram,the work done during a compression process is represented by the area under the curve.For a given change in volume,the adiabatic curve is steeper than the isothermal curve.Since the adiabatic curve lies above the isothermal curve for the same volume range during compression,the area under the adiabatic curve is greater than the area under the isothermal curve.Therefore,compressing the gas through an adiabatic process requires more work to be done than compressing it isothermally.

Class 11 Physics Thermodynamics Mix Examples-Thermodynamics

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$A$ 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 All NEET

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.

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An ideal gas goes through a reversible cycle $a \to b \to c \to d$ and has the $V - T$ diagram shown below. Processes $d \to a$ and $b \to c$ are adiabatic. The corresponding $P - V$ diagram for the process is (all figures are schematic and not drawn to scale):

MediumJEE MAIN 2015

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$A$ gas obeying the equation of state $pV = RT$ undergoes a hypothetical reversible process described by the equation $pV^{5/3} \exp \left(-\frac{pV}{E_0}\right) = C_1$,where $C_1$ and $E_0$ are dimensioned constants. Then,for this process,the thermal compressibility at high temperature

KVPY 2017

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Two identical adiabatic vessels are filled with oxygen at pressure $P_1$ and $P_2$ $(P_1 > P_2)$. The vessels are interconnected with each other by a non-conducting pipe. If $U_{01}$ and $U_{02}$ denote the initial internal energy of oxygen in the first and second vessel respectively,and $U_{f1}$ and $U_{f2}$ denote the final internal energy values,then:

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An ideal gas is subjected to a cyclic process involving four thermodynamic states. The amounts of heat $(Q)$ and work $(W)$ involved in each of these states are:
$Q_1 = 6000 \ J, Q_2 = -5500 \ J, Q_3 = -3000 \ J, Q_4 = 3500 \ J$
$W_1 = 2500 \ J, W_2 = -1000 \ J, W_3 = -1200 \ J, W_4 = x \ J$
The ratio of the net work done by the gas to the total heat absorbed by the gas is $\eta$. The values of $x$ and $\eta$ respectively are:

DifficultTS EAMCET 2009

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Two identical samples of a gas are allowed to expand $(i)$ isothermally and $(ii)$ adiabatically. The work done is:

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$A$ 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

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An ideal gas goes through a reversible cycle $a \to b \to c \to d$ and has the $V - T$ diagram shown below. Processes $d \to a$ and $b \to c$ are adiabatic. The corresponding $P - V$ diagram for the process is (all figures are schematic and not drawn to scale):

$A$ gas obeying the equation of state $pV = RT$ undergoes a hypothetical reversible process described by the equation $pV^{5/3} \exp \left(-\frac{pV}{E_0}\right) = C_1$,where $C_1$ and $E_0$ are dimensioned constants. Then,for this process,the thermal compressibility at high temperature

Two identical samples of a gas are allowed to expand $(i)$ isothermally and $(ii)$ adiabatically. The work done is:

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