139023
Let speed of sound at $0^{0} \mathrm{C}$ be $332 \mathrm{~ms}^{-1}$. On a winter day sound travels $342 \mathrm{~ms}^{-1}$ in one second. The atmospheric temperature on that day is:
139024
If pressure and temperature of an ideal gas are doubled and volume is halved, the number of molecules of gas
1 Becomes half
2 Becomes two times
3 Becomes four times
4 Remain constant
Explanation:
A From ideal gas equation, $\mathrm{PV}=\mathrm{nRT}$ $\mathrm{n}=\frac{\mathrm{PV}}{\mathrm{RT}}$ It is given as pressure and temperature of the ideal gas is doubled and Volume of the ideal gas is halved $\mathrm{P}=2 \mathrm{P}, \mathrm{V}=\frac{\mathrm{V}}{2} \text { and } \mathrm{T}=2 \mathrm{~T}$ $2 \mathrm{P} \times \frac{\mathrm{V}}{2}=\mathrm{nRT} \times 2$ $\mathrm{P} \times \mathrm{V}=\mathrm{nRT} \times 2$ $\mathrm{n}=\frac{\mathrm{PV}}{2 \times \mathrm{RT}}$ From this it is clear that, number of molecules or moles is halved when the pressure and temperature are double and volume is halved.
JCECE-2017
Kinetic Theory of Gases
139025
p-V diagram of an ideal gas is shown. The gas undergoes from initial state $A$ to final state $B$ such that initial and final volumes are same. Select the correct alternative for given process AB.
1 Work done by gas is positive
2 Work done by gas is negative
3 Temperature of gas increases continuously
4 Process is isochoric
Explanation:
B As we can see that the volume does not remain constant throughout the process. Therefore, the process is not isochoric. Now, the work done in this process will be given by the area in this graph which has been mentioned in the above graph. The process is in anti-clockwise direction that is why the area will be negative. Thus, the work done by gas will also be negative.
UPSEE - 2017
Kinetic Theory of Gases
139026
If the pressure and the volume of certain quantity of ideal gas are halved, then its temperature
1 is doubled
2 becomes one-fourth
3 remains constant
4 is halved
5 become four times
Explanation:
B The equation for an ideal gas is given by- $\mathrm{PV}=\mathrm{nRT}$ Here, the pressure and volume of certain quantity is getting halved, $\therefore \quad \frac{\mathrm{P}}{2} \times \frac{\mathrm{V}}{2}=\mathrm{nRT}^{\prime}$ $\frac{\mathrm{PV}}{4}=\mathrm{nRT}^{\prime}$ From equation (i), $\frac{\mathrm{nRT}}{4}=\mathrm{nRT}^{\prime}$ $\mathrm{T}^{\prime}=\frac{\mathrm{T}}{4}$ Hence, the temperature of ideal gas becomes one fourth.
139023
Let speed of sound at $0^{0} \mathrm{C}$ be $332 \mathrm{~ms}^{-1}$. On a winter day sound travels $342 \mathrm{~ms}^{-1}$ in one second. The atmospheric temperature on that day is:
139024
If pressure and temperature of an ideal gas are doubled and volume is halved, the number of molecules of gas
1 Becomes half
2 Becomes two times
3 Becomes four times
4 Remain constant
Explanation:
A From ideal gas equation, $\mathrm{PV}=\mathrm{nRT}$ $\mathrm{n}=\frac{\mathrm{PV}}{\mathrm{RT}}$ It is given as pressure and temperature of the ideal gas is doubled and Volume of the ideal gas is halved $\mathrm{P}=2 \mathrm{P}, \mathrm{V}=\frac{\mathrm{V}}{2} \text { and } \mathrm{T}=2 \mathrm{~T}$ $2 \mathrm{P} \times \frac{\mathrm{V}}{2}=\mathrm{nRT} \times 2$ $\mathrm{P} \times \mathrm{V}=\mathrm{nRT} \times 2$ $\mathrm{n}=\frac{\mathrm{PV}}{2 \times \mathrm{RT}}$ From this it is clear that, number of molecules or moles is halved when the pressure and temperature are double and volume is halved.
JCECE-2017
Kinetic Theory of Gases
139025
p-V diagram of an ideal gas is shown. The gas undergoes from initial state $A$ to final state $B$ such that initial and final volumes are same. Select the correct alternative for given process AB.
1 Work done by gas is positive
2 Work done by gas is negative
3 Temperature of gas increases continuously
4 Process is isochoric
Explanation:
B As we can see that the volume does not remain constant throughout the process. Therefore, the process is not isochoric. Now, the work done in this process will be given by the area in this graph which has been mentioned in the above graph. The process is in anti-clockwise direction that is why the area will be negative. Thus, the work done by gas will also be negative.
UPSEE - 2017
Kinetic Theory of Gases
139026
If the pressure and the volume of certain quantity of ideal gas are halved, then its temperature
1 is doubled
2 becomes one-fourth
3 remains constant
4 is halved
5 become four times
Explanation:
B The equation for an ideal gas is given by- $\mathrm{PV}=\mathrm{nRT}$ Here, the pressure and volume of certain quantity is getting halved, $\therefore \quad \frac{\mathrm{P}}{2} \times \frac{\mathrm{V}}{2}=\mathrm{nRT}^{\prime}$ $\frac{\mathrm{PV}}{4}=\mathrm{nRT}^{\prime}$ From equation (i), $\frac{\mathrm{nRT}}{4}=\mathrm{nRT}^{\prime}$ $\mathrm{T}^{\prime}=\frac{\mathrm{T}}{4}$ Hence, the temperature of ideal gas becomes one fourth.
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Kinetic Theory of Gases
139023
Let speed of sound at $0^{0} \mathrm{C}$ be $332 \mathrm{~ms}^{-1}$. On a winter day sound travels $342 \mathrm{~ms}^{-1}$ in one second. The atmospheric temperature on that day is:
139024
If pressure and temperature of an ideal gas are doubled and volume is halved, the number of molecules of gas
1 Becomes half
2 Becomes two times
3 Becomes four times
4 Remain constant
Explanation:
A From ideal gas equation, $\mathrm{PV}=\mathrm{nRT}$ $\mathrm{n}=\frac{\mathrm{PV}}{\mathrm{RT}}$ It is given as pressure and temperature of the ideal gas is doubled and Volume of the ideal gas is halved $\mathrm{P}=2 \mathrm{P}, \mathrm{V}=\frac{\mathrm{V}}{2} \text { and } \mathrm{T}=2 \mathrm{~T}$ $2 \mathrm{P} \times \frac{\mathrm{V}}{2}=\mathrm{nRT} \times 2$ $\mathrm{P} \times \mathrm{V}=\mathrm{nRT} \times 2$ $\mathrm{n}=\frac{\mathrm{PV}}{2 \times \mathrm{RT}}$ From this it is clear that, number of molecules or moles is halved when the pressure and temperature are double and volume is halved.
JCECE-2017
Kinetic Theory of Gases
139025
p-V diagram of an ideal gas is shown. The gas undergoes from initial state $A$ to final state $B$ such that initial and final volumes are same. Select the correct alternative for given process AB.
1 Work done by gas is positive
2 Work done by gas is negative
3 Temperature of gas increases continuously
4 Process is isochoric
Explanation:
B As we can see that the volume does not remain constant throughout the process. Therefore, the process is not isochoric. Now, the work done in this process will be given by the area in this graph which has been mentioned in the above graph. The process is in anti-clockwise direction that is why the area will be negative. Thus, the work done by gas will also be negative.
UPSEE - 2017
Kinetic Theory of Gases
139026
If the pressure and the volume of certain quantity of ideal gas are halved, then its temperature
1 is doubled
2 becomes one-fourth
3 remains constant
4 is halved
5 become four times
Explanation:
B The equation for an ideal gas is given by- $\mathrm{PV}=\mathrm{nRT}$ Here, the pressure and volume of certain quantity is getting halved, $\therefore \quad \frac{\mathrm{P}}{2} \times \frac{\mathrm{V}}{2}=\mathrm{nRT}^{\prime}$ $\frac{\mathrm{PV}}{4}=\mathrm{nRT}^{\prime}$ From equation (i), $\frac{\mathrm{nRT}}{4}=\mathrm{nRT}^{\prime}$ $\mathrm{T}^{\prime}=\frac{\mathrm{T}}{4}$ Hence, the temperature of ideal gas becomes one fourth.
139023
Let speed of sound at $0^{0} \mathrm{C}$ be $332 \mathrm{~ms}^{-1}$. On a winter day sound travels $342 \mathrm{~ms}^{-1}$ in one second. The atmospheric temperature on that day is:
139024
If pressure and temperature of an ideal gas are doubled and volume is halved, the number of molecules of gas
1 Becomes half
2 Becomes two times
3 Becomes four times
4 Remain constant
Explanation:
A From ideal gas equation, $\mathrm{PV}=\mathrm{nRT}$ $\mathrm{n}=\frac{\mathrm{PV}}{\mathrm{RT}}$ It is given as pressure and temperature of the ideal gas is doubled and Volume of the ideal gas is halved $\mathrm{P}=2 \mathrm{P}, \mathrm{V}=\frac{\mathrm{V}}{2} \text { and } \mathrm{T}=2 \mathrm{~T}$ $2 \mathrm{P} \times \frac{\mathrm{V}}{2}=\mathrm{nRT} \times 2$ $\mathrm{P} \times \mathrm{V}=\mathrm{nRT} \times 2$ $\mathrm{n}=\frac{\mathrm{PV}}{2 \times \mathrm{RT}}$ From this it is clear that, number of molecules or moles is halved when the pressure and temperature are double and volume is halved.
JCECE-2017
Kinetic Theory of Gases
139025
p-V diagram of an ideal gas is shown. The gas undergoes from initial state $A$ to final state $B$ such that initial and final volumes are same. Select the correct alternative for given process AB.
1 Work done by gas is positive
2 Work done by gas is negative
3 Temperature of gas increases continuously
4 Process is isochoric
Explanation:
B As we can see that the volume does not remain constant throughout the process. Therefore, the process is not isochoric. Now, the work done in this process will be given by the area in this graph which has been mentioned in the above graph. The process is in anti-clockwise direction that is why the area will be negative. Thus, the work done by gas will also be negative.
UPSEE - 2017
Kinetic Theory of Gases
139026
If the pressure and the volume of certain quantity of ideal gas are halved, then its temperature
1 is doubled
2 becomes one-fourth
3 remains constant
4 is halved
5 become four times
Explanation:
B The equation for an ideal gas is given by- $\mathrm{PV}=\mathrm{nRT}$ Here, the pressure and volume of certain quantity is getting halved, $\therefore \quad \frac{\mathrm{P}}{2} \times \frac{\mathrm{V}}{2}=\mathrm{nRT}^{\prime}$ $\frac{\mathrm{PV}}{4}=\mathrm{nRT}^{\prime}$ From equation (i), $\frac{\mathrm{nRT}}{4}=\mathrm{nRT}^{\prime}$ $\mathrm{T}^{\prime}=\frac{\mathrm{T}}{4}$ Hence, the temperature of ideal gas becomes one fourth.
