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Kinetic Theory of Gases

139175 According to the assumption made in the kinetic theory of gases, when two molecules of a gas collide with each other then

1 neither K.E. nor momentum is conserved.

2 both K.E. and momentum are conserved.

3 momentum is conserved but K.E. is not conserved.

4 K.E. is conserved but momentum is not conserved.

MHT-CET 2020

Kinetic Theory of Gases

139177 Mean free path of molecules in a polyatomic gas is independent of

1 number density of the molecules

2 volume of the molecule

3 temperature of the gas

4 gas constant

R

Explanation:

D The mean free path of a gas molecule is the average distance between two successive collisions mean path of molecule is represent $λ$ .
$λ = \frac{1}{\sqrt{2} \cdot π d^{2} n}$
Where, $d =$ Diameter of molecule
$n =$ Number of molecule per unit volume
Mean free path of molecule is depends on number of the molecules, volume of molecule and temperature of gas.

TS- EAMCET-14.09.2020

Kinetic Theory of Gases

139181 If the average kinetic energy of a molecule of a hydrogen gas at $300 K$ is $E$ , then the average kinetic energy of a molecule of a nitrogen gas at the same temperature is

1

7 E

2

E / 14

3

14 E

4

E / 7

5

E

Explanation:

E We know that, average translational kinetic energy of gas molecule $= \frac{3}{2} K_{B} T$
$K.E. \propto T (∵ K_{B} = \frac{R}{N_{A}})$
Given, a molecule of a hydrogen gas (K.E) $= E$
Then, the kinetic energy of a molecule of $N_{2}$ gas $= E$

AP EAMCET (18.09.2020) Shift-I

Kinetic Theory of Gases

139188 The ratio of R.M.S. velocities of hydrogen molecules to oxygen molecules at $273^{\circ} C$ is (molecular wt. of hydrogen and oxygen is 2 and 32 respectively.

1

1 : 8

2

16 : 1

3

1 : 4

4

4 : 1

Explanation:

D We know that,
${(v_{rms})}_{O_{2}} = \sqrt{\frac{3 RT}{M_{O 2}}}$
${(v_{rms})}_{H_{2}} = \sqrt{\frac{3 RT}{M_{H 2}}}$
$\frac{{(v_{rms})}_{H_{2}}}{{(v_{rms})}_{O_{2}}} = \sqrt{\frac{M_{O_{2}}}{M_{H_{2}}}} = \sqrt{\frac{32}{2}} = \frac{4}{1}$
${(v_{rms})}_{H_{2}} : {(v_{rms})}_{O_{2}} = 4 : 1$

MHT-CET 2019

Kinetic Theory of Gases

139175 According to the assumption made in the kinetic theory of gases, when two molecules of a gas collide with each other then

1 neither K.E. nor momentum is conserved.

2 both K.E. and momentum are conserved.

3 momentum is conserved but K.E. is not conserved.

4 K.E. is conserved but momentum is not conserved.

MHT-CET 2020

Kinetic Theory of Gases

139177 Mean free path of molecules in a polyatomic gas is independent of

1 number density of the molecules

2 volume of the molecule

3 temperature of the gas

4 gas constant

R

Explanation:

D The mean free path of a gas molecule is the average distance between two successive collisions mean path of molecule is represent $λ$ .
$λ = \frac{1}{\sqrt{2} \cdot π d^{2} n}$
Where, $d =$ Diameter of molecule
$n =$ Number of molecule per unit volume
Mean free path of molecule is depends on number of the molecules, volume of molecule and temperature of gas.

TS- EAMCET-14.09.2020

Kinetic Theory of Gases

139181 If the average kinetic energy of a molecule of a hydrogen gas at $300 K$ is $E$ , then the average kinetic energy of a molecule of a nitrogen gas at the same temperature is

1

7 E

2

E / 14

3

14 E

4

E / 7

5

E

Explanation:

E We know that, average translational kinetic energy of gas molecule $= \frac{3}{2} K_{B} T$
$K.E. \propto T (∵ K_{B} = \frac{R}{N_{A}})$
Given, a molecule of a hydrogen gas (K.E) $= E$
Then, the kinetic energy of a molecule of $N_{2}$ gas $= E$

AP EAMCET (18.09.2020) Shift-I

Kinetic Theory of Gases

139188 The ratio of R.M.S. velocities of hydrogen molecules to oxygen molecules at $273^{\circ} C$ is (molecular wt. of hydrogen and oxygen is 2 and 32 respectively.

1

1 : 8

2

16 : 1

3

1 : 4

4

4 : 1

Explanation:

D We know that,
${(v_{rms})}_{O_{2}} = \sqrt{\frac{3 RT}{M_{O 2}}}$
${(v_{rms})}_{H_{2}} = \sqrt{\frac{3 RT}{M_{H 2}}}$
$\frac{{(v_{rms})}_{H_{2}}}{{(v_{rms})}_{O_{2}}} = \sqrt{\frac{M_{O_{2}}}{M_{H_{2}}}} = \sqrt{\frac{32}{2}} = \frac{4}{1}$
${(v_{rms})}_{H_{2}} : {(v_{rms})}_{O_{2}} = 4 : 1$

MHT-CET 2019

Kinetic Theory of Gases

139175 According to the assumption made in the kinetic theory of gases, when two molecules of a gas collide with each other then

1 neither K.E. nor momentum is conserved.

2 both K.E. and momentum are conserved.

3 momentum is conserved but K.E. is not conserved.

4 K.E. is conserved but momentum is not conserved.

MHT-CET 2020

Kinetic Theory of Gases

139177 Mean free path of molecules in a polyatomic gas is independent of

1 number density of the molecules

2 volume of the molecule

3 temperature of the gas

4 gas constant

R

Explanation:

D The mean free path of a gas molecule is the average distance between two successive collisions mean path of molecule is represent $λ$ .
$λ = \frac{1}{\sqrt{2} \cdot π d^{2} n}$
Where, $d =$ Diameter of molecule
$n =$ Number of molecule per unit volume
Mean free path of molecule is depends on number of the molecules, volume of molecule and temperature of gas.

TS- EAMCET-14.09.2020

Kinetic Theory of Gases

139181 If the average kinetic energy of a molecule of a hydrogen gas at $300 K$ is $E$ , then the average kinetic energy of a molecule of a nitrogen gas at the same temperature is

1

7 E

2

E / 14

3

14 E

4

E / 7

5

E

Explanation:

E We know that, average translational kinetic energy of gas molecule $= \frac{3}{2} K_{B} T$
$K.E. \propto T (∵ K_{B} = \frac{R}{N_{A}})$
Given, a molecule of a hydrogen gas (K.E) $= E$
Then, the kinetic energy of a molecule of $N_{2}$ gas $= E$

AP EAMCET (18.09.2020) Shift-I

Kinetic Theory of Gases

139188 The ratio of R.M.S. velocities of hydrogen molecules to oxygen molecules at $273^{\circ} C$ is (molecular wt. of hydrogen and oxygen is 2 and 32 respectively.

1

1 : 8

2

16 : 1

3

1 : 4

4

4 : 1

Explanation:

D We know that,
${(v_{rms})}_{O_{2}} = \sqrt{\frac{3 RT}{M_{O 2}}}$
${(v_{rms})}_{H_{2}} = \sqrt{\frac{3 RT}{M_{H 2}}}$
$\frac{{(v_{rms})}_{H_{2}}}{{(v_{rms})}_{O_{2}}} = \sqrt{\frac{M_{O_{2}}}{M_{H_{2}}}} = \sqrt{\frac{32}{2}} = \frac{4}{1}$
${(v_{rms})}_{H_{2}} : {(v_{rms})}_{O_{2}} = 4 : 1$

MHT-CET 2019

Kinetic Theory of Gases

139175 According to the assumption made in the kinetic theory of gases, when two molecules of a gas collide with each other then

1 neither K.E. nor momentum is conserved.

2 both K.E. and momentum are conserved.

3 momentum is conserved but K.E. is not conserved.

4 K.E. is conserved but momentum is not conserved.

MHT-CET 2020

Kinetic Theory of Gases

139177 Mean free path of molecules in a polyatomic gas is independent of

1 number density of the molecules

2 volume of the molecule

3 temperature of the gas

4 gas constant

R

Explanation:

D The mean free path of a gas molecule is the average distance between two successive collisions mean path of molecule is represent $λ$ .
$λ = \frac{1}{\sqrt{2} \cdot π d^{2} n}$
Where, $d =$ Diameter of molecule
$n =$ Number of molecule per unit volume
Mean free path of molecule is depends on number of the molecules, volume of molecule and temperature of gas.

TS- EAMCET-14.09.2020

Kinetic Theory of Gases

139181 If the average kinetic energy of a molecule of a hydrogen gas at $300 K$ is $E$ , then the average kinetic energy of a molecule of a nitrogen gas at the same temperature is

1

7 E

2

E / 14

3

14 E

4

E / 7

5

E

Explanation:

E We know that, average translational kinetic energy of gas molecule $= \frac{3}{2} K_{B} T$
$K.E. \propto T (∵ K_{B} = \frac{R}{N_{A}})$
Given, a molecule of a hydrogen gas (K.E) $= E$
Then, the kinetic energy of a molecule of $N_{2}$ gas $= E$

AP EAMCET (18.09.2020) Shift-I

Kinetic Theory of Gases

139188 The ratio of R.M.S. velocities of hydrogen molecules to oxygen molecules at $273^{\circ} C$ is (molecular wt. of hydrogen and oxygen is 2 and 32 respectively.

1

1 : 8

2

16 : 1

3

1 : 4

4

4 : 1

Explanation:

D We know that,
${(v_{rms})}_{O_{2}} = \sqrt{\frac{3 RT}{M_{O 2}}}$
${(v_{rms})}_{H_{2}} = \sqrt{\frac{3 RT}{M_{H 2}}}$
$\frac{{(v_{rms})}_{H_{2}}}{{(v_{rms})}_{O_{2}}} = \sqrt{\frac{M_{O_{2}}}{M_{H_{2}}}} = \sqrt{\frac{32}{2}} = \frac{4}{1}$
${(v_{rms})}_{H_{2}} : {(v_{rms})}_{O_{2}} = 4 : 1$

MHT-CET 2019

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