Kinetic Theory Test

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Kinetic Theory Test - 44

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Question 1
1 / -0

Kinetic energy of a gas molecule depends on :

A
Volume

B
Temperature

C
Pressure

D
None of these

Solution

According to law of equipartion of energy among molecules of a gas $$\dfrac{1}{2}KT$$ energy is distributed foe each degree of freedom $$(f).$$
For instance $$=K.E$$ of translation motion of a gas molecule with $$f=3$$
$$\Rightarrow K.E=\dfrac{3}{2}KT$$ thus $$K.E\propto T.$$
Hence, the answer is temperature.
Question 2
1 / -0

Rate of diffusion is:

A
Faster in liquids than in solids and gases

B
Faster in gases than in liquids and solids

C
Faster in solids than in liquids and gases

D
None of these

Solution

Rate of diffusion is faster in gas because inter molecular attraction is comparatively less in gases.So they are very free to move as compared to solid materials.
Question 3
1 / -0

Which of the following postulate of kinetic theory of matter states that collisions are perfectly elastic?

A
Gas molecules are in constant random motion

B
When collisions occur, the molecules lose no kinetic energy

C
Molecules can collide with each other and with the walls of the container

D
All of above

Solution

When collisions occur, the molecules lose no kinetic energy; that is, the collisions are said to be perfectly elastic. The total kinetic energy of all the molecules remains constant unless there is some outside interference.

Hence, the correct option is $$\text{B}$$
Question 4
1 / -0

Which of the following is a postulate of kinetic theory of matter?

A
All gases at a given temperature have the same average kinetic energy.

B
Lighter gas molecules move faster than heavier molecules.

C
The kinetic energy of a gas is a measure of its Kelvin temperature.

D
All of the above

Solution

All the above statements are postulates of kinetic theory of matter. The kinetic energy of a gas is a measure of its Kelvin temperature. Individual gas molecules have different speeds, but the temperature and kinetic energy of the gas refer to the average of these speeds. All gases at a given temperature have the same average kinetic energy. Lighter gas molecules move faster than heavier molecules.
Question 5
1 / -0

The molecules of gases are independent of each other bacause:

A
the molecules exert force of attraction

B
molecules exert force of repulsion

C
both a and b

D
molecules exert no force of attraction or repulsion

Solution

The kinetic theory of matter recognizes that matter is composed of very small particles. The molecules exert no force of attraction or repulsion upon one another, i.e., the molecules are independent of each other. This is the reason gases do not have a definite shape.
Question 6
1 / -0

The average kinetic energy of all the molecules is assumed to be:

A
inversely proportional to the absolute temperature of the gas

B
directly proportional to the absolute temperature and size of the gas

C
directly proportional to the absolute temperature of the gas

D
not related to the absolute temperature of the gas

Solution

The average kinetic energy of all the molecules is assumed to be directly proportional to the absolute temperature of the gas. This means that molecules of different gases at the same temperature have the same average kinetic energy. The kinetic energy of a moving molecule, like that of any moving object, is the energy associated with its motion.
Question 7
1 / -0

The gases carbon-monoxide $$(CO)$$ and nitrogen at the same temperature have kinetic energies $${E}_{1}$$ and $${E}_{2}$$ respectively. Then

A
$${E}_{1}=E_2$$

B
$${E}_{1}> {E}_{2}$$

C
$${E}_{1}< {E}_{2}$$

D
$${E}_{1}$$ and $${E}_{2}$$ cannot be compared

Solution

The gases carbon monoxide ($$CO$$) and nitrogen ($${N}_{2}$$) are diatomic, so both have equal kinetic energy $$\cfrac{5}{2}kT$$, ie., $${E}_{1}={E}_{2}$$
Question 8
1 / -0

A flask contains argon and chlorine in the ratio of $$2:1$$ by mass. The temperature of the mixture is $$27^0C$$. The ratio of average kinetic energies of two gases per molecule is

A
$$1:1$$

B
$$2:1$$

C
$$3:1$$

D
$$6:1$$

Solution

The average translational kinetic energy (per molecule) of any (ideal) gas (be it monatomic like argon, diatomic like chlorine or polyatomic) is always equal to $$\dfrac{3}{2}k_BT $$. It depends only on temperature and is independent of the nature of the gas.
Since argon and chlorine both have the same temperature in the flask, the ratio of average kinetic energy (per molecule) of the two gases is $$1:1$$.
Question 9
1 / -0

$$3$$ moles of mono-atomic gas ($$\gamma=5/3$$) is mixed with $$1$$ mole of a diatomic gas ($$\gamma=7/3$$). The value of $$\gamma$$ for the mixture will be

A
$$\cfrac{9}{11}$$

B
$$\cfrac{11}{7}$$

C
$$\cfrac{12}{7}$$

D
$$\cfrac{15}{7}$$

Solution

The number of degrees of freedom for the mixture is:
$$\quad { f }_{ mix }=\cfrac { { n }_{ 1 }{ f }_{ 1 }+{ n }_{ 2 }{ f }_{ 2 } }{ { n }_{ 1 }-{ n }_{ 2 } } $$$$=\cfrac { 3\times 3+1\times 5 }{ 4 } =\cfrac { 7 }{ 2 } $$
$$\quad \therefore \gamma =1+\cfrac { 2 }{ f } \quad \Rightarrow \gamma =1+\cfrac { 4 }{ 7 } =\cfrac { 11 }{ 7 } $$
Question 10
1 / -0

The kinetic particle theory explains the:

A
properties of the different states of matter

B
size and rigidity of different states of matter

C
reaction of matter

D
all of above

Solution

The kinetic particle theory explains the properties of the different states of matter. The particles in solids, liquids and gases have different amounts of energy. They are arranged differently and move in different ways.

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Kinetic Theory Test - 44

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Kinetic Theory Test - 44

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Question 1

Volume

Temperature

Pressure

None of these

Solution

Question 2

Faster in liquids than in solids and gases

Faster in gases than in liquids and solids

Faster in solids than in liquids and gases

None of these

Solution

Question 3

Gas molecules are in constant random motion

When collisions occur, the molecules lose no kinetic energy

Molecules can collide with each other and with the walls of the container

All of above

Solution

Question 4

All gases at a given temperature have the same average kinetic energy.

Lighter gas molecules move faster than heavier molecules.

The kinetic energy of a gas is a measure of its Kelvin temperature.

All of the above

Solution

Question 5

the molecules exert force of attraction

molecules exert force of repulsion

both a and b

molecules exert no force of attraction or repulsion

Solution

Question 6

inversely proportional to the absolute temperature of the gas

directly proportional to the absolute temperature and size of the gas

directly proportional to the absolute temperature of the gas

not related to the absolute temperature of the gas

Solution

Question 7

$${E}_{1}=E_2$$

$${E}_{1}> {E}_{2}$$

$${E}_{1}< {E}_{2}$$

$${E}_{1}$$ and $${E}_{2}$$ cannot be compared

Solution

Question 8

$$1:1$$

$$2:1$$

$$3:1$$

$$6:1$$

Solution

Question 9

$$\cfrac{9}{11}$$

$$\cfrac{11}{7}$$

$$\cfrac{12}{7}$$

$$\cfrac{15}{7}$$

Solution

Question 10

properties of the different states of matter

size and rigidity of different states of matter

reaction of matter

all of above

Solution

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