148484 An ideal gas undergoes four different processes from the same initial state as shown in the figure below. Those processes are adiabatic, isothermal, isobaric and isochoric. The curve which represents the adiabatic process among $1,2,3$ and 4 is

148485 Given below are two statements
Statement-I: When $\mu$ amount of an ideal gas undergoes adiabatic change from state $\left(P_{1}, V_{1}\right.$, $\left.T_{1}\right)$ to state $\left(P_{2}, V_{2}, T_{2}\right)$, then work done is $\mathbf{W}=\frac{\operatorname{IR}\left(\mathbf{T}_{2}-\mathbf{T}_{1}\right)}{1-\gamma}$, where $\gamma=\frac{\mathbf{C}_{\mathbf{p}}}{\mathbf{C}_{\mathrm{v}}}$ and $\mathbf{R}=$ universal gas constant.
Statement-II : In the above case, when work is done on the gas, the temperature of the gas would rise.
Choose the correct answer from the options given below

148486 Two moles of a monoatomic gas at $27^{\circ} \mathrm{C}$ and three moles of a diatomic gas at the same temperature expand adiabatically. If the work done by each gas during the expansion is $4157 \mathrm{~J}$, The ratio of the final temperatures of the monoatomic gas to that of the diatomic gas is
$\text { (Universal gas constant }=\mathbf{8 . 3 1 4} \mathrm{Jmol}^{-1} \mathrm{~K}^{-1} \text { ) }$

148487 A gas is expanded from an initial state to a final along a path on a P-V diagram. The path consists of (i) an isothermal expansion of work $50 \mathrm{~J}$. If the internal energy of gas is changed by $-30 \mathrm{~J}$, then the work done by gas during adiabatic expansion is

148484 An ideal gas undergoes four different processes from the same initial state as shown in the figure below. Those processes are adiabatic, isothermal, isobaric and isochoric. The curve which represents the adiabatic process among $1,2,3$ and 4 is

148485 Given below are two statements
Statement-I: When $\mu$ amount of an ideal gas undergoes adiabatic change from state $\left(P_{1}, V_{1}\right.$, $\left.T_{1}\right)$ to state $\left(P_{2}, V_{2}, T_{2}\right)$, then work done is $\mathbf{W}=\frac{\operatorname{IR}\left(\mathbf{T}_{2}-\mathbf{T}_{1}\right)}{1-\gamma}$, where $\gamma=\frac{\mathbf{C}_{\mathbf{p}}}{\mathbf{C}_{\mathrm{v}}}$ and $\mathbf{R}=$ universal gas constant.
Statement-II : In the above case, when work is done on the gas, the temperature of the gas would rise.
Choose the correct answer from the options given below

148486 Two moles of a monoatomic gas at $27^{\circ} \mathrm{C}$ and three moles of a diatomic gas at the same temperature expand adiabatically. If the work done by each gas during the expansion is $4157 \mathrm{~J}$, The ratio of the final temperatures of the monoatomic gas to that of the diatomic gas is
$\text { (Universal gas constant }=\mathbf{8 . 3 1 4} \mathrm{Jmol}^{-1} \mathrm{~K}^{-1} \text { ) }$

148487 A gas is expanded from an initial state to a final along a path on a P-V diagram. The path consists of (i) an isothermal expansion of work $50 \mathrm{~J}$. If the internal energy of gas is changed by $-30 \mathrm{~J}$, then the work done by gas during adiabatic expansion is

148484 An ideal gas undergoes four different processes from the same initial state as shown in the figure below. Those processes are adiabatic, isothermal, isobaric and isochoric. The curve which represents the adiabatic process among $1,2,3$ and 4 is

148485 Given below are two statements
Statement-I: When $\mu$ amount of an ideal gas undergoes adiabatic change from state $\left(P_{1}, V_{1}\right.$, $\left.T_{1}\right)$ to state $\left(P_{2}, V_{2}, T_{2}\right)$, then work done is $\mathbf{W}=\frac{\operatorname{IR}\left(\mathbf{T}_{2}-\mathbf{T}_{1}\right)}{1-\gamma}$, where $\gamma=\frac{\mathbf{C}_{\mathbf{p}}}{\mathbf{C}_{\mathrm{v}}}$ and $\mathbf{R}=$ universal gas constant.
Statement-II : In the above case, when work is done on the gas, the temperature of the gas would rise.
Choose the correct answer from the options given below

148486 Two moles of a monoatomic gas at $27^{\circ} \mathrm{C}$ and three moles of a diatomic gas at the same temperature expand adiabatically. If the work done by each gas during the expansion is $4157 \mathrm{~J}$, The ratio of the final temperatures of the monoatomic gas to that of the diatomic gas is
$\text { (Universal gas constant }=\mathbf{8 . 3 1 4} \mathrm{Jmol}^{-1} \mathrm{~K}^{-1} \text { ) }$

148487 A gas is expanded from an initial state to a final along a path on a P-V diagram. The path consists of (i) an isothermal expansion of work $50 \mathrm{~J}$. If the internal energy of gas is changed by $-30 \mathrm{~J}$, then the work done by gas during adiabatic expansion is

148484 An ideal gas undergoes four different processes from the same initial state as shown in the figure below. Those processes are adiabatic, isothermal, isobaric and isochoric. The curve which represents the adiabatic process among $1,2,3$ and 4 is

148485 Given below are two statements
Statement-I: When $\mu$ amount of an ideal gas undergoes adiabatic change from state $\left(P_{1}, V_{1}\right.$, $\left.T_{1}\right)$ to state $\left(P_{2}, V_{2}, T_{2}\right)$, then work done is $\mathbf{W}=\frac{\operatorname{IR}\left(\mathbf{T}_{2}-\mathbf{T}_{1}\right)}{1-\gamma}$, where $\gamma=\frac{\mathbf{C}_{\mathbf{p}}}{\mathbf{C}_{\mathrm{v}}}$ and $\mathbf{R}=$ universal gas constant.
Statement-II : In the above case, when work is done on the gas, the temperature of the gas would rise.
Choose the correct answer from the options given below

148486 Two moles of a monoatomic gas at $27^{\circ} \mathrm{C}$ and three moles of a diatomic gas at the same temperature expand adiabatically. If the work done by each gas during the expansion is $4157 \mathrm{~J}$, The ratio of the final temperatures of the monoatomic gas to that of the diatomic gas is
$\text { (Universal gas constant }=\mathbf{8 . 3 1 4} \mathrm{Jmol}^{-1} \mathrm{~K}^{-1} \text { ) }$

148487 A gas is expanded from an initial state to a final along a path on a P-V diagram. The path consists of (i) an isothermal expansion of work $50 \mathrm{~J}$. If the internal energy of gas is changed by $-30 \mathrm{~J}$, then the work done by gas during adiabatic expansion is