One mole of an ideal gas undergoes a cyclic process, consisting of two isochores and two isobars. Temperature at $1$ and $3$ equal to $T_1$ and $T_3$ respectively. The work done by the gas over the cycle, if the point $2$ and $4$ lie on the same isotherm
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A perfect gas of a given mass is heated first in a small vessel and then in a large vessel, such that their volumes remain unchanged. The $P-T$ curves are
A gas may expand either adiabatically or isothermally. A number of $P-V$ curves are drawn for the two processes over different range of pressure and volume. It will be found that
A cylinder of mass $1\,kg$ is given heat of $20000\, J$ at atmospheric pressure. If initially temperature of cylinder is $20\,^oC$, then work done by the cylinder will be .......$J$ (Given that Specific heat of cylinder $= 400 \,J\, kg^{-1}$, Coefficient of volume expansion $= 9 \times {10^{-5}}\,^o C^{-1}$, Atmospheric pressure $= 10^5 \,N/m^2$ and density of cylinder $9000\,kg/m^3$)
An ideal gas undergoes a circular cycle centred at $4 \,atm , 4 L$ as shown in the diagram. The maximum temperature attained in this process is close to
Consider two containers $A$ and $B$ containing monoatomic gases at the same Pressure $(P)$, Volume $(V)$ and Temperature $(T)$. The gas in $A$ is compressed isothermally to $\frac{1}{8}$ of its original volume while the gas $B$ is compressed adiabatically to $\frac{1}{8}$ of its original volume. The ratio of final pressure of gas in $B$ to that of gas in $A$ is ...........
$0.02\, moles$ of an ideal diatomic gas with initial temperature $20^{\circ} C$ is compressed from $1500 \,cm ^{3}$ to $500 \,cm ^{3}$. The thermodynamic process is such that $p V^{2}=\beta$, where $\beta$ is a constant. Then, the value of $\beta$ is close to (the gas constant, $R=8.31 \,J / K / mol$ ).
One mole of an ideal gas $(\gamma = 1.4)$ is adiabatically compressed so that its temperature rises from $27\,^oC$ to $35\,^oC$. The change in the internal energy of the gas is .... $J$ (given $R = 8.3 \,J/mole/K$)