(A) The work done $W$ in different thermodynamic processes is given by:$1$. Isothermal process: $W = \int_{V_1}^{V_2} P dV = \mu RT \ln(\frac{V_2}{V_1

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(A) The work done $W$ in different thermodynamic processes is given by:$1$. Isothermal process: $W = \int_{V_1}^{V_2} P dV = \mu RT \ln(\frac{V_2}{V_1})$. Thus,$i-c$.$2$. Isobaric process: Pressure $P$ is constant,so $W = P \int_{V_1}^{V_2} dV = P(V_2 - V_1)$. Thus,$ii-d$.$3$. Isochoric process: Volume $V$ is constant,so $dV = 0$,which implies $W = 0$. Thus,$iii-a$.$4$. Adiabatic process: $W = \frac{P_1 V_1 - P_2 V_2}{\gamma - 1} = \frac{1}{\gamma - 1}[P_2 V_2 - P_1 V_1]$ (with a sign convention adjustment). Thus,$iv-b$.Therefore,the correct matching is $i-c, ii-d, iii-a, iv-b$.

Class 11 Physics Thermodynamics Mix Examples-Thermodynamics

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Match the following:
List-$I$ List-$II$
$i)$ Isothermal process $a)$ $0$
$ii)$ Isobaric process $b)$ $\frac{1}{\gamma-1}[P_2 V_2 - P_1 V_1]$
$iii)$ Isochoric process $c)$ $\mu RT \ln(\frac{V_2}{V_1})$
$iv)$ Adiabatic process $d)$ $P(V_2 - V_1)$

The correct answer is:

AP EAMCET 2017 All AP EAMCET

A
$i-c, ii-d, iii-a, iv-b$
B
$i-a, ii-d, iii-b, iv-c$
C
$i-c, ii-b, iii-d, iv-a$
D
$i-b, ii-c, iii-a, iv-d$

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For the given $P-V$ diagram of a thermodynamic system,match the curves with their respective thermodynamic processes. ($P$ = Pressure and $V$ = Volume)
Curve Process
$I$ $a)$ Adiabatic
$II$ $b)$ Isobaric
$III$ $c)$ Isochoric
$IV$ $d)$ Isothermal

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List-$I$	List-$II$
$i)$ Isothermal process	$a)$ $0$
$ii)$ Isobaric process	$b)$ $\frac{1}{\gamma-1}[P_2 V_2 - P_1 V_1]$
$iii)$ Isochoric process	$c)$ $\mu RT \ln(\frac{V_2}{V_1})$
$iv)$ Adiabatic process	$d)$ $P(V_2 - V_1)$

Curve	Process
$I$	$a)$ Adiabatic
$II$	$b)$ Isobaric
$III$	$c)$ Isochoric
$IV$	$d)$ Isothermal

Match the following:List-$I$List-$II$$i)$ Isothermal process$a)$ $0$$ii)$ Isobaric process$b)$ $\frac{1}{\gamma-1}[P_2 V_2 - P_1 V_1]$$iii)$ Isochoric process$c)$ $\mu RT \ln(\frac{V_2}{V_1})$$iv)$ Adiabatic process$d)$ $P(V_2 - V_1)$The correct answer is:

Similar Questions

One mole of an ideal gas goes from an initial state $A$ to a final state $B$ via two processes: It first undergoes isothermal expansion from volume $V$ to $3V$ and then its volume is reduced from $3V$ to $V$ at constant pressure. The correct $P-V$ diagram representing the two processes is:

For the given $P-V$ diagram of a thermodynamic system,match the curves with their respective thermodynamic processes. ($P$ = Pressure and $V$ = Volume)CurveProcess$I$$a)$ Adiabatic$II$$b)$ Isobaric$III$$c)$ Isochoric$IV$$d)$ Isothermal

Given $P_A = 3 \times 10^4 \, Pa$,$P_B = 8 \times 10^4 \, Pa$,$V_A = 2 \times 10^{-3} \, m^3$,and $V_D = 5 \times 10^{-3} \, m^3$. An ideal gas absorbs $600 \, J$ of heat in the process $AB$ and $200 \, J$ of heat in the process $BC$. Find the change in internal energy between $A$ and $C$ in $J$.

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Match the following:
List-$I$ List-$II$
$i)$ Isothermal process $a)$ $0$
$ii)$ Isobaric process $b)$ $\frac{1}{\gamma-1}[P_2 V_2 - P_1 V_1]$
$iii)$ Isochoric process $c)$ $\mu RT \ln(\frac{V_2}{V_1})$
$iv)$ Adiabatic process $d)$ $P(V_2 - V_1)$

The correct answer is:

For the given $P-V$ diagram of a thermodynamic system,match the curves with their respective thermodynamic processes. ($P$ = Pressure and $V$ = Volume)
Curve Process
$I$ $a)$ Adiabatic
$II$ $b)$ Isobaric
$III$ $c)$ Isochoric
$IV$ $d)$ Isothermal