371504
An ideal gas expand isothermally from a volume \(V_{1}\) to \(V_{2}\) and then compressed to original volume \(V_{1}\) adiabatically. Initial pressure is \(P_{1}\) and finally pressure is \(P_{3}\). The total work done is \(W\). Then
1 \(P_{3} < P_{1}, W < 0\)
2 \(P_{3} < P_{1}, W>0\)
3 \(P_{3}=P_{1}, W=0\)
4 \(P_{3}>P_{1}, W < 0\)
Explanation:
From graph it is clear that \(P_{3}>P_{1}\).
Since area under adiabatic process \((BCED)\) is greater than that of isothermal process \((ABDE)\). Therefore net work done \(\begin{aligned}& W=W_{A B}+W_{B C} \\& W_{A B}=(+) v e ; W_{B C}=(-) v e \Rightarrow W=(-) v e\end{aligned}\)
PHXI12:THERMODYNAMICS
371505
A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process untill its volume is again reduced to half. Then,
1 Compressing the gas isothermally will require more work to be done.
2 Compressing the gas through adiabatic process will require more work to be done.
3 Compressing the gas isothermally or adiabatically will require the same amount of work.
4 Which of the case(whether compressing through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.
Explanation:
\({W_{ext}} = \) negative of area with volume-axis
\(W\) ( adiabatic ) > \(W\) ( isothermal )
NEET - 2016
PHXI12:THERMODYNAMICS
371506
If \(\gamma\) denotes the ratio of two specific heats of gas, the ratio of slope of adiabatic and isothermal \(\mathrm{PV}\) curves at their point of intersection is
1 \(\gamma\)
2 \(\gamma / 1\)
3 \(\gamma+1\)
4 \(\gamma-1\)
Explanation:
Slope of adiabatic curve \(=\gamma \times\) (Slope of isothermal curve)
PHXI12:THERMODYNAMICS
371507
An ideal gas is compressed to \(\dfrac{1}{4} t h\) its initial volume by means of several process. Which of the process results in the maximum work done on the gas?
1 Isobaric
2 Adiabatic
3 Isobaric
4 Isochoric
Explanation:
Work done \(=\) Negative of area under \(P - V\) curve So, largest work takes place in adiabatic process.
371504
An ideal gas expand isothermally from a volume \(V_{1}\) to \(V_{2}\) and then compressed to original volume \(V_{1}\) adiabatically. Initial pressure is \(P_{1}\) and finally pressure is \(P_{3}\). The total work done is \(W\). Then
1 \(P_{3} < P_{1}, W < 0\)
2 \(P_{3} < P_{1}, W>0\)
3 \(P_{3}=P_{1}, W=0\)
4 \(P_{3}>P_{1}, W < 0\)
Explanation:
From graph it is clear that \(P_{3}>P_{1}\).
Since area under adiabatic process \((BCED)\) is greater than that of isothermal process \((ABDE)\). Therefore net work done \(\begin{aligned}& W=W_{A B}+W_{B C} \\& W_{A B}=(+) v e ; W_{B C}=(-) v e \Rightarrow W=(-) v e\end{aligned}\)
PHXI12:THERMODYNAMICS
371505
A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process untill its volume is again reduced to half. Then,
1 Compressing the gas isothermally will require more work to be done.
2 Compressing the gas through adiabatic process will require more work to be done.
3 Compressing the gas isothermally or adiabatically will require the same amount of work.
4 Which of the case(whether compressing through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.
Explanation:
\({W_{ext}} = \) negative of area with volume-axis
\(W\) ( adiabatic ) > \(W\) ( isothermal )
NEET - 2016
PHXI12:THERMODYNAMICS
371506
If \(\gamma\) denotes the ratio of two specific heats of gas, the ratio of slope of adiabatic and isothermal \(\mathrm{PV}\) curves at their point of intersection is
1 \(\gamma\)
2 \(\gamma / 1\)
3 \(\gamma+1\)
4 \(\gamma-1\)
Explanation:
Slope of adiabatic curve \(=\gamma \times\) (Slope of isothermal curve)
PHXI12:THERMODYNAMICS
371507
An ideal gas is compressed to \(\dfrac{1}{4} t h\) its initial volume by means of several process. Which of the process results in the maximum work done on the gas?
1 Isobaric
2 Adiabatic
3 Isobaric
4 Isochoric
Explanation:
Work done \(=\) Negative of area under \(P - V\) curve So, largest work takes place in adiabatic process.
371504
An ideal gas expand isothermally from a volume \(V_{1}\) to \(V_{2}\) and then compressed to original volume \(V_{1}\) adiabatically. Initial pressure is \(P_{1}\) and finally pressure is \(P_{3}\). The total work done is \(W\). Then
1 \(P_{3} < P_{1}, W < 0\)
2 \(P_{3} < P_{1}, W>0\)
3 \(P_{3}=P_{1}, W=0\)
4 \(P_{3}>P_{1}, W < 0\)
Explanation:
From graph it is clear that \(P_{3}>P_{1}\).
Since area under adiabatic process \((BCED)\) is greater than that of isothermal process \((ABDE)\). Therefore net work done \(\begin{aligned}& W=W_{A B}+W_{B C} \\& W_{A B}=(+) v e ; W_{B C}=(-) v e \Rightarrow W=(-) v e\end{aligned}\)
PHXI12:THERMODYNAMICS
371505
A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process untill its volume is again reduced to half. Then,
1 Compressing the gas isothermally will require more work to be done.
2 Compressing the gas through adiabatic process will require more work to be done.
3 Compressing the gas isothermally or adiabatically will require the same amount of work.
4 Which of the case(whether compressing through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.
Explanation:
\({W_{ext}} = \) negative of area with volume-axis
\(W\) ( adiabatic ) > \(W\) ( isothermal )
NEET - 2016
PHXI12:THERMODYNAMICS
371506
If \(\gamma\) denotes the ratio of two specific heats of gas, the ratio of slope of adiabatic and isothermal \(\mathrm{PV}\) curves at their point of intersection is
1 \(\gamma\)
2 \(\gamma / 1\)
3 \(\gamma+1\)
4 \(\gamma-1\)
Explanation:
Slope of adiabatic curve \(=\gamma \times\) (Slope of isothermal curve)
PHXI12:THERMODYNAMICS
371507
An ideal gas is compressed to \(\dfrac{1}{4} t h\) its initial volume by means of several process. Which of the process results in the maximum work done on the gas?
1 Isobaric
2 Adiabatic
3 Isobaric
4 Isochoric
Explanation:
Work done \(=\) Negative of area under \(P - V\) curve So, largest work takes place in adiabatic process.
371504
An ideal gas expand isothermally from a volume \(V_{1}\) to \(V_{2}\) and then compressed to original volume \(V_{1}\) adiabatically. Initial pressure is \(P_{1}\) and finally pressure is \(P_{3}\). The total work done is \(W\). Then
1 \(P_{3} < P_{1}, W < 0\)
2 \(P_{3} < P_{1}, W>0\)
3 \(P_{3}=P_{1}, W=0\)
4 \(P_{3}>P_{1}, W < 0\)
Explanation:
From graph it is clear that \(P_{3}>P_{1}\).
Since area under adiabatic process \((BCED)\) is greater than that of isothermal process \((ABDE)\). Therefore net work done \(\begin{aligned}& W=W_{A B}+W_{B C} \\& W_{A B}=(+) v e ; W_{B C}=(-) v e \Rightarrow W=(-) v e\end{aligned}\)
PHXI12:THERMODYNAMICS
371505
A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process untill its volume is again reduced to half. Then,
1 Compressing the gas isothermally will require more work to be done.
2 Compressing the gas through adiabatic process will require more work to be done.
3 Compressing the gas isothermally or adiabatically will require the same amount of work.
4 Which of the case(whether compressing through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.
Explanation:
\({W_{ext}} = \) negative of area with volume-axis
\(W\) ( adiabatic ) > \(W\) ( isothermal )
NEET - 2016
PHXI12:THERMODYNAMICS
371506
If \(\gamma\) denotes the ratio of two specific heats of gas, the ratio of slope of adiabatic and isothermal \(\mathrm{PV}\) curves at their point of intersection is
1 \(\gamma\)
2 \(\gamma / 1\)
3 \(\gamma+1\)
4 \(\gamma-1\)
Explanation:
Slope of adiabatic curve \(=\gamma \times\) (Slope of isothermal curve)
PHXI12:THERMODYNAMICS
371507
An ideal gas is compressed to \(\dfrac{1}{4} t h\) its initial volume by means of several process. Which of the process results in the maximum work done on the gas?
1 Isobaric
2 Adiabatic
3 Isobaric
4 Isochoric
Explanation:
Work done \(=\) Negative of area under \(P - V\) curve So, largest work takes place in adiabatic process.
