138942
If there is a straight line parallel to volume axis in a $\mathrm{P}-\mathrm{V}$ diagram, then it is a..... graph.
1 Isochoric
2 Isobaric
3 Isothermal
4 None of these
Explanation:
B As shown in the figure below - Process $\mathrm{AB}$ on $\mathrm{PV}$ diagram is constant pressure process and constant pressure process is known as isobaric process.
UP CPMT-2003
Kinetic Theory of Gases
138946
At constant volume temperature is increased, then
1 Collision of walls will be less
2 Number of collisions per unit time will increase
3 Collisions will be in straight lines
4 Collisions will not change
Explanation:
B Ideal gas equation $\mathrm{PV}=\mathrm{nRT}$ For constant volume $\mathrm{P} \propto \mathrm{T}$ $\therefore$ When the temperature is increased, the pressure will also be increase. Now, We know that, the pressure of a gas is directly proportional to the number of collisions. So, an increase in temperature results in an increase of pressure and hence the number of collisions increases.
AIPMT 1989
Kinetic Theory of Gases
138963
The internal energy of a gram-molecule of an ideal gas depends on
1 Pressure alone
2 Volume alone
3 Temperature alone
4 Both on pressure as well as on temperature
Explanation:
C We know that, $\Delta \mathrm{U}=\mathrm{nC}_{\mathrm{v}} \Delta \mathrm{T}$ $\Delta \mathrm{U}=\text { Internal energy }$ Hence, Internal Energy of an Ideal gas possess translation Kinetic Energy. So, internal energy only depends on temperature
Shift-II
Kinetic Theory of Gases
138915
In the kinetic theory of gases, it is assumed that the gas molecules:
1 Repel each other
2 Collide elastically
3 Move with uniform velocity
4 Are massless particle
Explanation:
B In the kinetic theory of gases, the collision between the molecules and the walls are perfectly elastic. That means when the molecules collide they do not loss kinetic energy.
138942
If there is a straight line parallel to volume axis in a $\mathrm{P}-\mathrm{V}$ diagram, then it is a..... graph.
1 Isochoric
2 Isobaric
3 Isothermal
4 None of these
Explanation:
B As shown in the figure below - Process $\mathrm{AB}$ on $\mathrm{PV}$ diagram is constant pressure process and constant pressure process is known as isobaric process.
UP CPMT-2003
Kinetic Theory of Gases
138946
At constant volume temperature is increased, then
1 Collision of walls will be less
2 Number of collisions per unit time will increase
3 Collisions will be in straight lines
4 Collisions will not change
Explanation:
B Ideal gas equation $\mathrm{PV}=\mathrm{nRT}$ For constant volume $\mathrm{P} \propto \mathrm{T}$ $\therefore$ When the temperature is increased, the pressure will also be increase. Now, We know that, the pressure of a gas is directly proportional to the number of collisions. So, an increase in temperature results in an increase of pressure and hence the number of collisions increases.
AIPMT 1989
Kinetic Theory of Gases
138963
The internal energy of a gram-molecule of an ideal gas depends on
1 Pressure alone
2 Volume alone
3 Temperature alone
4 Both on pressure as well as on temperature
Explanation:
C We know that, $\Delta \mathrm{U}=\mathrm{nC}_{\mathrm{v}} \Delta \mathrm{T}$ $\Delta \mathrm{U}=\text { Internal energy }$ Hence, Internal Energy of an Ideal gas possess translation Kinetic Energy. So, internal energy only depends on temperature
Shift-II
Kinetic Theory of Gases
138915
In the kinetic theory of gases, it is assumed that the gas molecules:
1 Repel each other
2 Collide elastically
3 Move with uniform velocity
4 Are massless particle
Explanation:
B In the kinetic theory of gases, the collision between the molecules and the walls are perfectly elastic. That means when the molecules collide they do not loss kinetic energy.
138942
If there is a straight line parallel to volume axis in a $\mathrm{P}-\mathrm{V}$ diagram, then it is a..... graph.
1 Isochoric
2 Isobaric
3 Isothermal
4 None of these
Explanation:
B As shown in the figure below - Process $\mathrm{AB}$ on $\mathrm{PV}$ diagram is constant pressure process and constant pressure process is known as isobaric process.
UP CPMT-2003
Kinetic Theory of Gases
138946
At constant volume temperature is increased, then
1 Collision of walls will be less
2 Number of collisions per unit time will increase
3 Collisions will be in straight lines
4 Collisions will not change
Explanation:
B Ideal gas equation $\mathrm{PV}=\mathrm{nRT}$ For constant volume $\mathrm{P} \propto \mathrm{T}$ $\therefore$ When the temperature is increased, the pressure will also be increase. Now, We know that, the pressure of a gas is directly proportional to the number of collisions. So, an increase in temperature results in an increase of pressure and hence the number of collisions increases.
AIPMT 1989
Kinetic Theory of Gases
138963
The internal energy of a gram-molecule of an ideal gas depends on
1 Pressure alone
2 Volume alone
3 Temperature alone
4 Both on pressure as well as on temperature
Explanation:
C We know that, $\Delta \mathrm{U}=\mathrm{nC}_{\mathrm{v}} \Delta \mathrm{T}$ $\Delta \mathrm{U}=\text { Internal energy }$ Hence, Internal Energy of an Ideal gas possess translation Kinetic Energy. So, internal energy only depends on temperature
Shift-II
Kinetic Theory of Gases
138915
In the kinetic theory of gases, it is assumed that the gas molecules:
1 Repel each other
2 Collide elastically
3 Move with uniform velocity
4 Are massless particle
Explanation:
B In the kinetic theory of gases, the collision between the molecules and the walls are perfectly elastic. That means when the molecules collide they do not loss kinetic energy.
138942
If there is a straight line parallel to volume axis in a $\mathrm{P}-\mathrm{V}$ diagram, then it is a..... graph.
1 Isochoric
2 Isobaric
3 Isothermal
4 None of these
Explanation:
B As shown in the figure below - Process $\mathrm{AB}$ on $\mathrm{PV}$ diagram is constant pressure process and constant pressure process is known as isobaric process.
UP CPMT-2003
Kinetic Theory of Gases
138946
At constant volume temperature is increased, then
1 Collision of walls will be less
2 Number of collisions per unit time will increase
3 Collisions will be in straight lines
4 Collisions will not change
Explanation:
B Ideal gas equation $\mathrm{PV}=\mathrm{nRT}$ For constant volume $\mathrm{P} \propto \mathrm{T}$ $\therefore$ When the temperature is increased, the pressure will also be increase. Now, We know that, the pressure of a gas is directly proportional to the number of collisions. So, an increase in temperature results in an increase of pressure and hence the number of collisions increases.
AIPMT 1989
Kinetic Theory of Gases
138963
The internal energy of a gram-molecule of an ideal gas depends on
1 Pressure alone
2 Volume alone
3 Temperature alone
4 Both on pressure as well as on temperature
Explanation:
C We know that, $\Delta \mathrm{U}=\mathrm{nC}_{\mathrm{v}} \Delta \mathrm{T}$ $\Delta \mathrm{U}=\text { Internal energy }$ Hence, Internal Energy of an Ideal gas possess translation Kinetic Energy. So, internal energy only depends on temperature
Shift-II
Kinetic Theory of Gases
138915
In the kinetic theory of gases, it is assumed that the gas molecules:
1 Repel each other
2 Collide elastically
3 Move with uniform velocity
4 Are massless particle
Explanation:
B In the kinetic theory of gases, the collision between the molecules and the walls are perfectly elastic. That means when the molecules collide they do not loss kinetic energy.
