NEET Test Series from KOTA - 10 Papers In MS WORD
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PHXI12:THERMODYNAMICS
371573
In the equation \(P{V^\gamma } = \)constant, the value of \(\gamma\) is unity. Then the process is
1 isothermal
2 adiabatic
3 isobaric
4 irreversible
Explanation:
\(PV = \) constant represents isothermal process.
PHXI12:THERMODYNAMICS
371574
When an ideal gas in a cylinder was compressed isothermally by a piston, the work done on the gas was found to be \(1.5 \times {10^4}\;J.\) During the process about
1 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
2 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
3 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
4 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
Explanation:
In isothermal compression, there is always an increase of heat which must flow out the gas. \(\Delta Q = \Delta U + \Delta W\) \( \Rightarrow \quad \Delta Q = \Delta W\quad (\because \Delta U = 0)\) \(\Delta Q = 1.5 \times {10^4}J = \frac{{1.5 \times {{10}^4}}}{{4.18}}cal\) \( = - 3.6 \times {10^3}cal\)
PHXI12:THERMODYNAMICS
371575
The internal energy of an ideal gas increases during an isothermal process when the gas is
1 expanded by adding more molecules to it
2 expanded by adding more heat to it
3 expanded against zero pressure
4 compressed by doing work on it
Explanation:
Internal energy of an ideal gas is given by \(U=\dfrac{f}{2} \mu R T\) where, \(f\) is degree of freedom. \( = \frac{f}{2}\left( {\frac{N}{{{N_A}}}} \right)RT\) \( \Rightarrow \quad U \propto NT\) In isothermal process, \(T=\) constant \(\Rightarrow \quad U \propto N\) i.e., internal energy increases by increasing number of molecules \(N\).
PHXI12:THERMODYNAMICS
371576
Statement A : The isothermal curves intersect each other at a certain point. Statement B : The isothermal changes takes place slowly, so the isothermal curves have very little slope.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Isothermal curves never intersect each other. Isothermal changes take place slowly, as they have a very little slope. So option (2) is correct.
371573
In the equation \(P{V^\gamma } = \)constant, the value of \(\gamma\) is unity. Then the process is
1 isothermal
2 adiabatic
3 isobaric
4 irreversible
Explanation:
\(PV = \) constant represents isothermal process.
PHXI12:THERMODYNAMICS
371574
When an ideal gas in a cylinder was compressed isothermally by a piston, the work done on the gas was found to be \(1.5 \times {10^4}\;J.\) During the process about
1 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
2 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
3 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
4 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
Explanation:
In isothermal compression, there is always an increase of heat which must flow out the gas. \(\Delta Q = \Delta U + \Delta W\) \( \Rightarrow \quad \Delta Q = \Delta W\quad (\because \Delta U = 0)\) \(\Delta Q = 1.5 \times {10^4}J = \frac{{1.5 \times {{10}^4}}}{{4.18}}cal\) \( = - 3.6 \times {10^3}cal\)
PHXI12:THERMODYNAMICS
371575
The internal energy of an ideal gas increases during an isothermal process when the gas is
1 expanded by adding more molecules to it
2 expanded by adding more heat to it
3 expanded against zero pressure
4 compressed by doing work on it
Explanation:
Internal energy of an ideal gas is given by \(U=\dfrac{f}{2} \mu R T\) where, \(f\) is degree of freedom. \( = \frac{f}{2}\left( {\frac{N}{{{N_A}}}} \right)RT\) \( \Rightarrow \quad U \propto NT\) In isothermal process, \(T=\) constant \(\Rightarrow \quad U \propto N\) i.e., internal energy increases by increasing number of molecules \(N\).
PHXI12:THERMODYNAMICS
371576
Statement A : The isothermal curves intersect each other at a certain point. Statement B : The isothermal changes takes place slowly, so the isothermal curves have very little slope.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Isothermal curves never intersect each other. Isothermal changes take place slowly, as they have a very little slope. So option (2) is correct.
371573
In the equation \(P{V^\gamma } = \)constant, the value of \(\gamma\) is unity. Then the process is
1 isothermal
2 adiabatic
3 isobaric
4 irreversible
Explanation:
\(PV = \) constant represents isothermal process.
PHXI12:THERMODYNAMICS
371574
When an ideal gas in a cylinder was compressed isothermally by a piston, the work done on the gas was found to be \(1.5 \times {10^4}\;J.\) During the process about
1 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
2 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
3 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
4 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
Explanation:
In isothermal compression, there is always an increase of heat which must flow out the gas. \(\Delta Q = \Delta U + \Delta W\) \( \Rightarrow \quad \Delta Q = \Delta W\quad (\because \Delta U = 0)\) \(\Delta Q = 1.5 \times {10^4}J = \frac{{1.5 \times {{10}^4}}}{{4.18}}cal\) \( = - 3.6 \times {10^3}cal\)
PHXI12:THERMODYNAMICS
371575
The internal energy of an ideal gas increases during an isothermal process when the gas is
1 expanded by adding more molecules to it
2 expanded by adding more heat to it
3 expanded against zero pressure
4 compressed by doing work on it
Explanation:
Internal energy of an ideal gas is given by \(U=\dfrac{f}{2} \mu R T\) where, \(f\) is degree of freedom. \( = \frac{f}{2}\left( {\frac{N}{{{N_A}}}} \right)RT\) \( \Rightarrow \quad U \propto NT\) In isothermal process, \(T=\) constant \(\Rightarrow \quad U \propto N\) i.e., internal energy increases by increasing number of molecules \(N\).
PHXI12:THERMODYNAMICS
371576
Statement A : The isothermal curves intersect each other at a certain point. Statement B : The isothermal changes takes place slowly, so the isothermal curves have very little slope.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Isothermal curves never intersect each other. Isothermal changes take place slowly, as they have a very little slope. So option (2) is correct.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
PHXI12:THERMODYNAMICS
371573
In the equation \(P{V^\gamma } = \)constant, the value of \(\gamma\) is unity. Then the process is
1 isothermal
2 adiabatic
3 isobaric
4 irreversible
Explanation:
\(PV = \) constant represents isothermal process.
PHXI12:THERMODYNAMICS
371574
When an ideal gas in a cylinder was compressed isothermally by a piston, the work done on the gas was found to be \(1.5 \times {10^4}\;J.\) During the process about
1 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
2 \(3.6 \times {10^3}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
3 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed into the gas
4 \(1.5 \times {10^4}{\mkern 1mu} {\mkern 1mu} cal\) of heat flowed out from the gas
Explanation:
In isothermal compression, there is always an increase of heat which must flow out the gas. \(\Delta Q = \Delta U + \Delta W\) \( \Rightarrow \quad \Delta Q = \Delta W\quad (\because \Delta U = 0)\) \(\Delta Q = 1.5 \times {10^4}J = \frac{{1.5 \times {{10}^4}}}{{4.18}}cal\) \( = - 3.6 \times {10^3}cal\)
PHXI12:THERMODYNAMICS
371575
The internal energy of an ideal gas increases during an isothermal process when the gas is
1 expanded by adding more molecules to it
2 expanded by adding more heat to it
3 expanded against zero pressure
4 compressed by doing work on it
Explanation:
Internal energy of an ideal gas is given by \(U=\dfrac{f}{2} \mu R T\) where, \(f\) is degree of freedom. \( = \frac{f}{2}\left( {\frac{N}{{{N_A}}}} \right)RT\) \( \Rightarrow \quad U \propto NT\) In isothermal process, \(T=\) constant \(\Rightarrow \quad U \propto N\) i.e., internal energy increases by increasing number of molecules \(N\).
PHXI12:THERMODYNAMICS
371576
Statement A : The isothermal curves intersect each other at a certain point. Statement B : The isothermal changes takes place slowly, so the isothermal curves have very little slope.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Isothermal curves never intersect each other. Isothermal changes take place slowly, as they have a very little slope. So option (2) is correct.