Advertisements
Advertisements
Question
Calculate the temperature at which the rms velocity of a gas triples its value at S.T.P. (standard temperature T1 = 273 K)
Advertisements
Solution
At STP temperature T1 = 273 K
RMS velocity of a gas, (vrms)1 = v
New RMS velocity of a gas, at temperature (T2)
New temperature T2 = ?
vrms = `sqrt((3"RT")/"M")`
`("v"_"rms")_1/("v"_"rms")_2 = sqrt("T"_1/"T"_2)`
T2 = `[("v"_"rms")_2/("v"_"rms")_1]^2 xx "T"_1`
= `((3"v")/"v")^2 xx 273`
= 9 × 273
T2 = 2457 K
APPEARS IN
RELATED QUESTIONS
The velocity of the three molecules is 2 km s-1, 4 km s-1, 6 km s-1. Find (i) mean square velocity (ii) root mean square velocity.
Why moon has no atmosphere?
Write the expression for rms speed, average speed and most probable speed of a gas molecule.
If the rms speed of methane gas in the Jupiter’s atmosphere is 471.8 ms−1, shows that the surface temperature of Jupiter is sub-zero.
The root mean square velocity of molecules of a gas is 200 m/s. What will be the root mean square velocity of the molecules, if the molecular weight is doubled and the absolute temperature is halved?
To what temperature should hydrogen at 227° C be cooled at constant pressure so that root mean square velocity of its molecule becomes half of its previous value?
Ratio of pressures exerted by two gases is 4 : 3 and their densities are in the ratio 3 : 4. The ratio of their R.M.S. velocities is ____________.
The temperature at which the molecules of nitrogen will have the same r.m.s. velocity as the molecules of oxygen at 327° C is ____________.
What will be the effect on the root mean square velocity of oxygen molecules if the temperature is doubled and the oxygen molecule dissociates into atomic oxygen?
Which of the following relations is correct for root means square speed of a gas at temperature T?
(m = mass of molecule, K = Boltzmann constant)
