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

  • 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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Similar Questions

Which of the following statements is true?

$A$ gas has temperature $T$ and volume $V$. At constant pressure,if the temperature is increased by $\Delta T$,the volume increases by $\Delta V$. How does $\delta = \frac{\Delta V}{V\Delta T}$ vary with temperature?

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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$STATEMENT-1$: The total translational kinetic energy of all the molecules of a given mass of an ideal gas is $1.5$ times the product of its pressure and its volume. Because
$STATEMENT-2$: The molecules of a gas collide with each other and the velocities of the molecules change due to the collision.

What is/are the same for $O_2$ and $NH_3$ in gaseous state?

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