139097
In a $p-V$ diagram for an ideal gas (where $p$ is along the $y$-axis and $V$ is along the $x$-axis), the value of the ratio : "Slope of the adiabatic curve/slope of the isothermal curve" at any point will be (where symbols have their usual meanings)
C $\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {adiabatic }}=\gamma\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {isotherml }}$ $\frac{\text { Slope of adiabatic curve }}{\text { Slope of Isothermal curve }}=\gamma$ $\frac{\mathrm{Cp}}{\mathrm{Cv}}=\gamma$
CG PET- 2005
Kinetic Theory of Gases
139098
The factor $R / N_{A}$ in an ideal gas law is
1 Celsius constant
2 Kelvin constant
3 Universal gas constant
4 Boltzmann's constant
Explanation:
D The factor $\frac{\mathrm{R}}{\mathrm{N}_{\mathrm{A}}}$ in an ideal gas law is Boltzmann's constant $\mathrm{R}$ is ideal gas constant and $\mathrm{N}_{\mathrm{A}}$ is Avogadro's number.
J and K-CET-2018
Kinetic Theory of Gases
138971
A closed compartment containing gas is moving with some acceleration in horizontal direction. Neglect effect of gravity. Then the pressure in the compartment is
1 same everywhere
2 lower in front side
3 lower in rear side
4 lower in upper side
Explanation:
B When the container is accelerated in the forward direction, a pseudo force will act on the gas molecules inside the container in the backward direction and thus the movement of majority of gas molecules in a container is directly proportional to its concentration. Since, the concentration of gas is lower on the forward side the pressure is lower there.
IIT JEE 1999
Kinetic Theory of Gases
139027
The value of $\frac{P V}{T}$ for one mole of an ideal gas is nearly equal to:
B An ideal gas is a gas which satisfy the assumption of the kinetic theory of gases. It is the equation of a hypothetical ideal gas and a good approximation of the behaviour of many gases under many conditions although it has many limitations.
$\text { So
Kinetic Theory of Gases
139029
A real gas behaves as an ideal gas
1 at very low pressure and high temperature
2 high pressure and low temperature
3 high temperature and high pressure
4 low pressure and low temperature
Explanation:
A A real gas behaves as an ideal gas at very low pressure and high temperature because it has zero volume of molecule and does not have intermolecular force. At very low pressure the volume of gas is large so that the volume of molecule is negligible compared to volume of gas and at very high temperature the kinetic energy of molecule is very large and the effect of intermolecular forces can be neglected. That is why the real gases behave as an ideal gas at low pressure and high temperature.
139097
In a $p-V$ diagram for an ideal gas (where $p$ is along the $y$-axis and $V$ is along the $x$-axis), the value of the ratio : "Slope of the adiabatic curve/slope of the isothermal curve" at any point will be (where symbols have their usual meanings)
C $\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {adiabatic }}=\gamma\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {isotherml }}$ $\frac{\text { Slope of adiabatic curve }}{\text { Slope of Isothermal curve }}=\gamma$ $\frac{\mathrm{Cp}}{\mathrm{Cv}}=\gamma$
CG PET- 2005
Kinetic Theory of Gases
139098
The factor $R / N_{A}$ in an ideal gas law is
1 Celsius constant
2 Kelvin constant
3 Universal gas constant
4 Boltzmann's constant
Explanation:
D The factor $\frac{\mathrm{R}}{\mathrm{N}_{\mathrm{A}}}$ in an ideal gas law is Boltzmann's constant $\mathrm{R}$ is ideal gas constant and $\mathrm{N}_{\mathrm{A}}$ is Avogadro's number.
J and K-CET-2018
Kinetic Theory of Gases
138971
A closed compartment containing gas is moving with some acceleration in horizontal direction. Neglect effect of gravity. Then the pressure in the compartment is
1 same everywhere
2 lower in front side
3 lower in rear side
4 lower in upper side
Explanation:
B When the container is accelerated in the forward direction, a pseudo force will act on the gas molecules inside the container in the backward direction and thus the movement of majority of gas molecules in a container is directly proportional to its concentration. Since, the concentration of gas is lower on the forward side the pressure is lower there.
IIT JEE 1999
Kinetic Theory of Gases
139027
The value of $\frac{P V}{T}$ for one mole of an ideal gas is nearly equal to:
B An ideal gas is a gas which satisfy the assumption of the kinetic theory of gases. It is the equation of a hypothetical ideal gas and a good approximation of the behaviour of many gases under many conditions although it has many limitations.
$\text { So
Kinetic Theory of Gases
139029
A real gas behaves as an ideal gas
1 at very low pressure and high temperature
2 high pressure and low temperature
3 high temperature and high pressure
4 low pressure and low temperature
Explanation:
A A real gas behaves as an ideal gas at very low pressure and high temperature because it has zero volume of molecule and does not have intermolecular force. At very low pressure the volume of gas is large so that the volume of molecule is negligible compared to volume of gas and at very high temperature the kinetic energy of molecule is very large and the effect of intermolecular forces can be neglected. That is why the real gases behave as an ideal gas at low pressure and high temperature.
139097
In a $p-V$ diagram for an ideal gas (where $p$ is along the $y$-axis and $V$ is along the $x$-axis), the value of the ratio : "Slope of the adiabatic curve/slope of the isothermal curve" at any point will be (where symbols have their usual meanings)
C $\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {adiabatic }}=\gamma\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {isotherml }}$ $\frac{\text { Slope of adiabatic curve }}{\text { Slope of Isothermal curve }}=\gamma$ $\frac{\mathrm{Cp}}{\mathrm{Cv}}=\gamma$
CG PET- 2005
Kinetic Theory of Gases
139098
The factor $R / N_{A}$ in an ideal gas law is
1 Celsius constant
2 Kelvin constant
3 Universal gas constant
4 Boltzmann's constant
Explanation:
D The factor $\frac{\mathrm{R}}{\mathrm{N}_{\mathrm{A}}}$ in an ideal gas law is Boltzmann's constant $\mathrm{R}$ is ideal gas constant and $\mathrm{N}_{\mathrm{A}}$ is Avogadro's number.
J and K-CET-2018
Kinetic Theory of Gases
138971
A closed compartment containing gas is moving with some acceleration in horizontal direction. Neglect effect of gravity. Then the pressure in the compartment is
1 same everywhere
2 lower in front side
3 lower in rear side
4 lower in upper side
Explanation:
B When the container is accelerated in the forward direction, a pseudo force will act on the gas molecules inside the container in the backward direction and thus the movement of majority of gas molecules in a container is directly proportional to its concentration. Since, the concentration of gas is lower on the forward side the pressure is lower there.
IIT JEE 1999
Kinetic Theory of Gases
139027
The value of $\frac{P V}{T}$ for one mole of an ideal gas is nearly equal to:
B An ideal gas is a gas which satisfy the assumption of the kinetic theory of gases. It is the equation of a hypothetical ideal gas and a good approximation of the behaviour of many gases under many conditions although it has many limitations.
$\text { So
Kinetic Theory of Gases
139029
A real gas behaves as an ideal gas
1 at very low pressure and high temperature
2 high pressure and low temperature
3 high temperature and high pressure
4 low pressure and low temperature
Explanation:
A A real gas behaves as an ideal gas at very low pressure and high temperature because it has zero volume of molecule and does not have intermolecular force. At very low pressure the volume of gas is large so that the volume of molecule is negligible compared to volume of gas and at very high temperature the kinetic energy of molecule is very large and the effect of intermolecular forces can be neglected. That is why the real gases behave as an ideal gas at low pressure and high temperature.
139097
In a $p-V$ diagram for an ideal gas (where $p$ is along the $y$-axis and $V$ is along the $x$-axis), the value of the ratio : "Slope of the adiabatic curve/slope of the isothermal curve" at any point will be (where symbols have their usual meanings)
C $\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {adiabatic }}=\gamma\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {isotherml }}$ $\frac{\text { Slope of adiabatic curve }}{\text { Slope of Isothermal curve }}=\gamma$ $\frac{\mathrm{Cp}}{\mathrm{Cv}}=\gamma$
CG PET- 2005
Kinetic Theory of Gases
139098
The factor $R / N_{A}$ in an ideal gas law is
1 Celsius constant
2 Kelvin constant
3 Universal gas constant
4 Boltzmann's constant
Explanation:
D The factor $\frac{\mathrm{R}}{\mathrm{N}_{\mathrm{A}}}$ in an ideal gas law is Boltzmann's constant $\mathrm{R}$ is ideal gas constant and $\mathrm{N}_{\mathrm{A}}$ is Avogadro's number.
J and K-CET-2018
Kinetic Theory of Gases
138971
A closed compartment containing gas is moving with some acceleration in horizontal direction. Neglect effect of gravity. Then the pressure in the compartment is
1 same everywhere
2 lower in front side
3 lower in rear side
4 lower in upper side
Explanation:
B When the container is accelerated in the forward direction, a pseudo force will act on the gas molecules inside the container in the backward direction and thus the movement of majority of gas molecules in a container is directly proportional to its concentration. Since, the concentration of gas is lower on the forward side the pressure is lower there.
IIT JEE 1999
Kinetic Theory of Gases
139027
The value of $\frac{P V}{T}$ for one mole of an ideal gas is nearly equal to:
B An ideal gas is a gas which satisfy the assumption of the kinetic theory of gases. It is the equation of a hypothetical ideal gas and a good approximation of the behaviour of many gases under many conditions although it has many limitations.
$\text { So
Kinetic Theory of Gases
139029
A real gas behaves as an ideal gas
1 at very low pressure and high temperature
2 high pressure and low temperature
3 high temperature and high pressure
4 low pressure and low temperature
Explanation:
A A real gas behaves as an ideal gas at very low pressure and high temperature because it has zero volume of molecule and does not have intermolecular force. At very low pressure the volume of gas is large so that the volume of molecule is negligible compared to volume of gas and at very high temperature the kinetic energy of molecule is very large and the effect of intermolecular forces can be neglected. That is why the real gases behave as an ideal gas at low pressure and high temperature.
139097
In a $p-V$ diagram for an ideal gas (where $p$ is along the $y$-axis and $V$ is along the $x$-axis), the value of the ratio : "Slope of the adiabatic curve/slope of the isothermal curve" at any point will be (where symbols have their usual meanings)
C $\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {adiabatic }}=\gamma\left|\frac{\mathrm{dp}}{\mathrm{dv}}\right|_{\text {isotherml }}$ $\frac{\text { Slope of adiabatic curve }}{\text { Slope of Isothermal curve }}=\gamma$ $\frac{\mathrm{Cp}}{\mathrm{Cv}}=\gamma$
CG PET- 2005
Kinetic Theory of Gases
139098
The factor $R / N_{A}$ in an ideal gas law is
1 Celsius constant
2 Kelvin constant
3 Universal gas constant
4 Boltzmann's constant
Explanation:
D The factor $\frac{\mathrm{R}}{\mathrm{N}_{\mathrm{A}}}$ in an ideal gas law is Boltzmann's constant $\mathrm{R}$ is ideal gas constant and $\mathrm{N}_{\mathrm{A}}$ is Avogadro's number.
J and K-CET-2018
Kinetic Theory of Gases
138971
A closed compartment containing gas is moving with some acceleration in horizontal direction. Neglect effect of gravity. Then the pressure in the compartment is
1 same everywhere
2 lower in front side
3 lower in rear side
4 lower in upper side
Explanation:
B When the container is accelerated in the forward direction, a pseudo force will act on the gas molecules inside the container in the backward direction and thus the movement of majority of gas molecules in a container is directly proportional to its concentration. Since, the concentration of gas is lower on the forward side the pressure is lower there.
IIT JEE 1999
Kinetic Theory of Gases
139027
The value of $\frac{P V}{T}$ for one mole of an ideal gas is nearly equal to:
B An ideal gas is a gas which satisfy the assumption of the kinetic theory of gases. It is the equation of a hypothetical ideal gas and a good approximation of the behaviour of many gases under many conditions although it has many limitations.
$\text { So
Kinetic Theory of Gases
139029
A real gas behaves as an ideal gas
1 at very low pressure and high temperature
2 high pressure and low temperature
3 high temperature and high pressure
4 low pressure and low temperature
Explanation:
A A real gas behaves as an ideal gas at very low pressure and high temperature because it has zero volume of molecule and does not have intermolecular force. At very low pressure the volume of gas is large so that the volume of molecule is negligible compared to volume of gas and at very high temperature the kinetic energy of molecule is very large and the effect of intermolecular forces can be neglected. That is why the real gases behave as an ideal gas at low pressure and high temperature.
