360294
The average kinetic energy of a helium atom at \(30^\circ C\) is
1 Less than \(1\,\,eV\)
2 A few \(k\,\,eV\)
3 \(50 - 60\,\,eV\)
4 \(13.6\,\,eV\)
Explanation:
Average kinetic energy \(E=\dfrac{F}{2} k T=\dfrac{3}{2} k T\) \( \Rightarrow E{\rm{ }} = \frac{3}{2} \times \left( {1.38 \times {{10}^{ - 23}}} \right)(273 + 30)\) \( = 6.27 \times {10^{ - 21}} J\) \( = 0.039\,eV < 1\,eV\)
PHXI13:KINETIC THEORY
360295
The mean energy of a molecule of an ideal gas is
1 \(kT\)
2 \(\frac{1}{2}kT\)
3 \(\frac{3}{2}kT\)
4 \(2\,kT\)
Explanation:
The mean energy of a molecule of an ideal gas is \(\frac{3}{2}kT\)
PHXI13:KINETIC THEORY
360296
A mixture of two gases consists of \(3\) moles of nitrogen and \(6\) moles of neon at temperature \(27^\circ C\). Neglecting all vibrational modes, the total internal energy of the system is \(\left( {R = 8.32\;J\;mo{l^{ - 1}}\;{K^{ - 1}}} \right)\)
360297
Pressure of an ideal gas is increased by keeping temperature constant. The kinetic energy of molecules
1 Decreases
2 Increases
3 Remains same
4 Increases or decreases depending on the nature of gas.
Explanation:
The kinetic energy of molecules of an ideal gas is \(K.E = \frac{3}{2}N{k_B}\,T\) From the above expression it is clear that \(\mathrm{E}\) depends on the temperature only. Thus, on increasing the pressure by keeping the temperature constant, the kinetic energy of molecules remains same.
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PHXI13:KINETIC THEORY
360294
The average kinetic energy of a helium atom at \(30^\circ C\) is
1 Less than \(1\,\,eV\)
2 A few \(k\,\,eV\)
3 \(50 - 60\,\,eV\)
4 \(13.6\,\,eV\)
Explanation:
Average kinetic energy \(E=\dfrac{F}{2} k T=\dfrac{3}{2} k T\) \( \Rightarrow E{\rm{ }} = \frac{3}{2} \times \left( {1.38 \times {{10}^{ - 23}}} \right)(273 + 30)\) \( = 6.27 \times {10^{ - 21}} J\) \( = 0.039\,eV < 1\,eV\)
PHXI13:KINETIC THEORY
360295
The mean energy of a molecule of an ideal gas is
1 \(kT\)
2 \(\frac{1}{2}kT\)
3 \(\frac{3}{2}kT\)
4 \(2\,kT\)
Explanation:
The mean energy of a molecule of an ideal gas is \(\frac{3}{2}kT\)
PHXI13:KINETIC THEORY
360296
A mixture of two gases consists of \(3\) moles of nitrogen and \(6\) moles of neon at temperature \(27^\circ C\). Neglecting all vibrational modes, the total internal energy of the system is \(\left( {R = 8.32\;J\;mo{l^{ - 1}}\;{K^{ - 1}}} \right)\)
360297
Pressure of an ideal gas is increased by keeping temperature constant. The kinetic energy of molecules
1 Decreases
2 Increases
3 Remains same
4 Increases or decreases depending on the nature of gas.
Explanation:
The kinetic energy of molecules of an ideal gas is \(K.E = \frac{3}{2}N{k_B}\,T\) From the above expression it is clear that \(\mathrm{E}\) depends on the temperature only. Thus, on increasing the pressure by keeping the temperature constant, the kinetic energy of molecules remains same.
360294
The average kinetic energy of a helium atom at \(30^\circ C\) is
1 Less than \(1\,\,eV\)
2 A few \(k\,\,eV\)
3 \(50 - 60\,\,eV\)
4 \(13.6\,\,eV\)
Explanation:
Average kinetic energy \(E=\dfrac{F}{2} k T=\dfrac{3}{2} k T\) \( \Rightarrow E{\rm{ }} = \frac{3}{2} \times \left( {1.38 \times {{10}^{ - 23}}} \right)(273 + 30)\) \( = 6.27 \times {10^{ - 21}} J\) \( = 0.039\,eV < 1\,eV\)
PHXI13:KINETIC THEORY
360295
The mean energy of a molecule of an ideal gas is
1 \(kT\)
2 \(\frac{1}{2}kT\)
3 \(\frac{3}{2}kT\)
4 \(2\,kT\)
Explanation:
The mean energy of a molecule of an ideal gas is \(\frac{3}{2}kT\)
PHXI13:KINETIC THEORY
360296
A mixture of two gases consists of \(3\) moles of nitrogen and \(6\) moles of neon at temperature \(27^\circ C\). Neglecting all vibrational modes, the total internal energy of the system is \(\left( {R = 8.32\;J\;mo{l^{ - 1}}\;{K^{ - 1}}} \right)\)
360297
Pressure of an ideal gas is increased by keeping temperature constant. The kinetic energy of molecules
1 Decreases
2 Increases
3 Remains same
4 Increases or decreases depending on the nature of gas.
Explanation:
The kinetic energy of molecules of an ideal gas is \(K.E = \frac{3}{2}N{k_B}\,T\) From the above expression it is clear that \(\mathrm{E}\) depends on the temperature only. Thus, on increasing the pressure by keeping the temperature constant, the kinetic energy of molecules remains same.
360294
The average kinetic energy of a helium atom at \(30^\circ C\) is
1 Less than \(1\,\,eV\)
2 A few \(k\,\,eV\)
3 \(50 - 60\,\,eV\)
4 \(13.6\,\,eV\)
Explanation:
Average kinetic energy \(E=\dfrac{F}{2} k T=\dfrac{3}{2} k T\) \( \Rightarrow E{\rm{ }} = \frac{3}{2} \times \left( {1.38 \times {{10}^{ - 23}}} \right)(273 + 30)\) \( = 6.27 \times {10^{ - 21}} J\) \( = 0.039\,eV < 1\,eV\)
PHXI13:KINETIC THEORY
360295
The mean energy of a molecule of an ideal gas is
1 \(kT\)
2 \(\frac{1}{2}kT\)
3 \(\frac{3}{2}kT\)
4 \(2\,kT\)
Explanation:
The mean energy of a molecule of an ideal gas is \(\frac{3}{2}kT\)
PHXI13:KINETIC THEORY
360296
A mixture of two gases consists of \(3\) moles of nitrogen and \(6\) moles of neon at temperature \(27^\circ C\). Neglecting all vibrational modes, the total internal energy of the system is \(\left( {R = 8.32\;J\;mo{l^{ - 1}}\;{K^{ - 1}}} \right)\)
360297
Pressure of an ideal gas is increased by keeping temperature constant. The kinetic energy of molecules
1 Decreases
2 Increases
3 Remains same
4 Increases or decreases depending on the nature of gas.
Explanation:
The kinetic energy of molecules of an ideal gas is \(K.E = \frac{3}{2}N{k_B}\,T\) From the above expression it is clear that \(\mathrm{E}\) depends on the temperature only. Thus, on increasing the pressure by keeping the temperature constant, the kinetic energy of molecules remains same.
