(A) According to the kinetic theory of gases,the pressure exerted by a gas is due to the collisions of gas molecules with the walls of the container,n

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The pressure exerted by a gas is due to the collisions between the molecules of the gas

(A) According to the kinetic theory of gases,the pressure exerted by a gas is due to the collisions of gas molecules with the walls of the container,not due to collisions between the molecules themselves.Therefore,statement $A$ is incorrect.Statement $B$ is a fundamental postulate of the kinetic theory.Statement $C$ is a standard assumption for an ideal gas.Statement $D$ is also a fundamental postulate,assuming no intermolecular forces exist except during collisions.

Class 11 Physics Kinetic Theory Mix Examples-Kinetic Theory of Gases

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According to the kinetic theory of gases,which of the following statements is $WRONG$?

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A
The pressure exerted by a gas is due to the collisions between the molecules of the gas
B
Collisions between the molecules of a gas and that of the molecules with the walls of the containers are perfectly elastic
C
All molecules of a gas are identical
D
The molecules do not exert appreciable force on one another except during collision

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Mix Examples-Kinetic Theory of Gases

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$A$ box contains $N$ molecules of a perfect gas at temperature ${T_1}$ and pressure ${P_1}$. The number of molecules in the box is doubled while keeping the total kinetic energy of the gas the same as before. If the new pressure is ${P_2}$ and temperature is ${T_2}$,then:

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$CO_2$ $(O-C-O)$ is a triatomic gas. The mean kinetic energy of one gram of the gas will be (where $N$ is Avogadro's number,$k$ is Boltzmann's constant,and the molecular weight of $CO_2 = 44$).

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The ratio of two specific heats of gas ${C_p}/{C_v}$ for argon is $1.6$ and for hydrogen is $1.4$. Adiabatic elasticity of argon at pressure $P$ is $E$. Adiabatic elasticity of hydrogen will also be equal to $E$ at the pressure

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$A$ thermally insulated vessel contains an ideal gas of molecular mass $M$ and ratio of specific heats $\gamma$. It is moving with speed $v$ and is suddenly brought to rest. Assuming no heat is lost to the surroundings,its temperature increases by

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An insulated container contains $4$ moles of an ideal diatomic gas at temperature $T$. Heat $Q$ is supplied to the gas,causing $2$ moles of the gas to dissociate into atoms. If the temperature of the gas remains constant,then:

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According to the kinetic theory of gases,which of the following statements is $WRONG$?

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$A$ box contains $N$ molecules of a perfect gas at temperature ${T_1}$ and pressure ${P_1}$. The number of molecules in the box is doubled while keeping the total kinetic energy of the gas the same as before. If the new pressure is ${P_2}$ and temperature is ${T_2}$,then:

$CO_2$ $(O-C-O)$ is a triatomic gas. The mean kinetic energy of one gram of the gas will be (where $N$ is Avogadro's number,$k$ is Boltzmann's constant,and the molecular weight of $CO_2 = 44$).

The ratio of two specific heats of gas ${C_p}/{C_v}$ for argon is $1.6$ and for hydrogen is $1.4$. Adiabatic elasticity of argon at pressure $P$ is $E$. Adiabatic elasticity of hydrogen will also be equal to $E$ at the pressure

$A$ thermally insulated vessel contains an ideal gas of molecular mass $M$ and ratio of specific heats $\gamma$. It is moving with speed $v$ and is suddenly brought to rest. Assuming no heat is lost to the surroundings,its temperature increases by

An insulated container contains $4$ moles of an ideal diatomic gas at temperature $T$. Heat $Q$ is supplied to the gas,causing $2$ moles of the gas to dissociate into atoms. If the temperature of the gas remains constant,then:

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