The rms velocity of H2 molecules at 27 $^{0}$ C is 1930 m/s. The rms velocity of O $_{2}$ molecules at 1200 K will be

365 m/s

No worries! We‘ve got your back. Try BYJU‘S free classes today!

965 m/s

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

765 m/s

No worries! We‘ve got your back. Try BYJU‘S free classes today!

865 m/s

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B 965 m/s
$C \propto \sqrt{\frac{T}{M}} C = k \sqrt{\frac{T}{M}} 1930 = k \sqrt{\frac{300}{2}} k = 157.55 C = 157.55 \sqrt{\frac{1200}{32}} C = 964.7 \approx 965 m / s$

Suggest Corrections

Similar questions

The molecules of a given mass of a gas have a rms velocity of 200 $m / s$ at $27^{\circ} C$ at a pressure of $1.0 \times 10^{5} N / m^{2}$ . When the temperature is $127^{\circ} C$ and pressure is $0.5 \times 10^{5} N / m^{2}$ , the rms velocity in $m / s$ will be:

If the rms speed of nitrogen molecules is $490 m s^{- 1}$ at 273K, find the rms speed of hydrogen molecules at the same temperature -

Q. RMS velocity of an ideal gas at

27^{o} C

500 m / s

, Temperature is increased four times, RMS velocity will become.

Q. For a given gas at

1 atm

pressure,

r m s

speed of the molecules is

200 m/s

127^{\circ} C

. At

2 atm

pressure and at

227^{\circ} C

, the

r m s

speed of the molecules will be

Join BYJU'S Learning Program

The rms velocity of H2 molecules at 270C is 1930 m/s. The rms velocity of O2 molecules at 1200 K will be

The correct option is B 965 m/sC∝√TMC=k√TM1930=k√3002k=157.55C=157.55√120032C=964.7≈965m/s

The rms velocity of H2 molecules at 27 $^{0}$ C is 1930 m/s. The rms velocity of O $_{2}$ molecules at 1200 K will be

The correct option is B 965 m/s
$C \propto \sqrt{\frac{T}{M}} C = k \sqrt{\frac{T}{M}} 1930 = k \sqrt{\frac{300}{2}} k = 157.55 C = 157.55 \sqrt{\frac{1200}{32}} C = 964.7 \approx 965 m / s$