At what temperature does the average translational kinetic energy of a molecule in a gas become equal to the kinetic energy of an electron accelerated from rest through a potential difference of $V$ volt? ($N=$ Avogadro number,$R=$ gas constant,$e=$ electronic charge)
- A$\frac{2 eVN}{3 R}$
- B$\frac{eVN}{R}$
- C$\frac{eVN}{4 R}$
- D$\frac{3 eVN}{2 R}$
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If $10^{22}$ gas molecules,each of mass $10^{-26} \ kg$,collide with a surface (perpendicular to it) elastically per second over an area of $1 \ m^2$ with a speed of $10^4 \ m/s$,the pressure exerted by the gas molecules will be of the order of:
If the number of molecules of ${H_2}$ is double that of ${O_2}$,then the ratio of the kinetic energy of hydrogen to that of oxygen at $300 \, K$ is:
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View SolutionThe kinetic energy of $20 \, L$ of ${H_2}$ gas is $1.5 \times 10^5 \, J$. Find the pressure exerted on the container.
Difficult
View Solution$A$ balloon has $5.0$ $g$ mole of helium at $7^{\circ} C$. Calculate
$(a)$ the number of atoms of helium in the balloon,
$(b)$ the total internal energy of the system.
$(a)$ the number of atoms of helium in the balloon,
$(b)$ the total internal energy of the system.
Medium
View SolutionThe 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 $kJ$)
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