Draw $P-V$ curves for isothermal and adiabatic processes of an ideal gas.
(N/A) The $P-V$ diagram represents a Carnot cycle,which consists of two isothermal processes and two adiabatic processes.
$1$. Isothermal expansion: The gas expands at a constant temperature.
$2$. Adiabatic expansion: The gas expands without any heat exchange with the surroundings.
$3$. Isothermal compression: The gas is compressed at a constant temperature.
$4$. Adiabatic compression: The gas is compressed without any heat exchange with the surroundings.
The adiabatic curves are steeper than the isothermal curves because the adiabatic bulk modulus is $\gamma$ times the isothermal bulk modulus,where $\gamma > 1$.
$1$. Isothermal expansion: The gas expands at a constant temperature.
$2$. Adiabatic expansion: The gas expands without any heat exchange with the surroundings.
$3$. Isothermal compression: The gas is compressed at a constant temperature.
$4$. Adiabatic compression: The gas is compressed without any heat exchange with the surroundings.
The adiabatic curves are steeper than the isothermal curves because the adiabatic bulk modulus is $\gamma$ times the isothermal bulk modulus,where $\gamma > 1$.
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Similar Questions
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:
$Q_1 = 6000 \ J, Q_2 = -5500 \ J, Q_3 = -3000 \ J, Q_4 = 3500 \ J$
$W_1 = 2500 \ J, W_2 = -1000 \ J, W_3 = -1200 \ J, W_4 = x \ J$
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:
DifficultAP EAMCET 2009
View SolutionMatch the following:
Column $I$ Column $II$ $A$. Ratio of $\frac{\Delta Q}{\Delta U}$ in an isobaric process $1$. $\frac{T_1}{T_1-T_2}$ $B$. Ratio of $\frac{\Delta Q}{\Delta W}$ in an isobaric process $2$. $\frac{T_2}{T_1-T_2}$ $C$. Coefficient of performance of a refrigerator $3$. $\frac{\gamma}{\gamma-1}$ $D$. Coefficient of performance of a heat pump $4$. $\gamma$
Codes:
$A \quad B \quad C \quad D$
| Column $I$ | Column $II$ |
| $A$. Ratio of $\frac{\Delta Q}{\Delta U}$ in an isobaric process | $1$. $\frac{T_1}{T_1-T_2}$ |
| $B$. Ratio of $\frac{\Delta Q}{\Delta W}$ in an isobaric process | $2$. $\frac{T_2}{T_1-T_2}$ |
| $C$. Coefficient of performance of a refrigerator | $3$. $\frac{\gamma}{\gamma-1}$ |
| $D$. Coefficient of performance of a heat pump | $4$. $\gamma$ |
Codes:
$A \quad B \quad C \quad D$
$A$ real gas within a closed chamber at $27^{\circ} C$ undergoes the cyclic process as shown in the figure. The gas obeys the $PV^3 = RT$ equation for the path $A$ to $B$. The net work done in the complete cycle is (assuming $R = 8 \, J/mol \cdot K$): (in $ \, J$)
DifficultJEE MAIN 2024
View SolutionThe $VT$ curve for a thermodynamic process is given. Identify the corresponding $PV$ curve.
$A$ monoatomic gas of $n$-moles is heated from temperature $T_1$ to $T_2$ under two different conditions: $(i)$ at constant volume and (ii) at constant pressure. The change in internal energy of the gas is
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