On the basis of the kinetic theory of gases,the gas exerts pressure because its molecules:
- Acontinuously lose their energy till it reaches the wall.
- Bare attracted by the walls of the container.
- Ccontinuously stick to the walls of the container.
- Dsuffer a change in momentum when they impinge on the walls of the container.
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Assertion $(A)$: The temperature of a gas is a result of the kinetic energy of its molecules.
Reason $(R)$: Due to kinetic energy,the molecules collide with each other to produce thermal energy.
Reason $(R)$: Due to kinetic energy,the molecules collide with each other to produce thermal energy.
The total internal energy of $4$ moles of a diatomic gas at a temperature of $27^{\circ} C$ is (Universal gas constant $R = 8.31 \ J \ mol^{-1} \ K^{-1}$) (in $kJ$)
The average translational kinetic energy of nitrogen (molar mass $28$) molecules at a particular temperature is $0.042 \ eV$. The translational kinetic energy of oxygen molecules (molar mass $32$) in $eV$ at double the temperature is:
If the average translational kinetic energy of a molecule in a gas is equal to the kinetic energy of an electron accelerating from rest through $10 \,V$, then the temperature of the gas molecule is (Boltzmann constant $= 1.38 \times 10^{-23} \,JK^{-1}$)
If the temperature of a gas is increased from $27^{\circ}C$ to $927^{\circ}C$,what will be the change in its kinetic energy?
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