The ratio of root mean square velocity to average velocity of a gas molecule at a particular temperature is.
At atmospheric pressure a nitrogen molecule therefore travels a distance of 59 nm between two collisions, while at ultra-high vacuum at pressures below 10-8 hPa it travels a distance of several kilometers. The relation between molecular number density and the mean free path is shown in a graph in Figure 1.5.
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Nov 30, 2016 · The rates of diffusion and effusion of a gas are both related to the root mean square (rms) velocity of the gas particles. For gases at the same temperature, this means that the rate of gas movement is inversely proportional to the square root of its molar mass.

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  • The root mean square speed of hydrogen molecules at 300 K is 1930 m/s. then the root mean square speed of oxygen molecules at 900 K will be (MHT-CET-2002) (a) 1930 m/s (b) 836 m/s (c) 643 m/s (d) m/s. Answer: (b) 9. A molecule of mass m moving with a velocity v makes 5 elastic collisions with a wall of the container per second.
  • Graham's law was the basis for separating uranium-235 from uranium-238 found in natural uraninite (uranium ore) during the Manhattan Project to build the first atomic bomb. The United States government built a gaseous diffusion plant at the Clinton Engineer Works in Oak Ridge, Tennessee, at the cost of $479 million (equivalent to $5.5 billion in 2019).

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Calculate the root mean square velocity and kinetic energy of F 2 , Cl 2 , and Br 2 at 298 K. Rank these three halogens with respect to their rate of effusion. 84 . Calculate the root mean square velocity and kinetic energy of CO, CO 2 , and SO 3 at 298 K.

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  • Example 7: Place the following gases all at the same T in order from slowest root mean square velocity to fastest root mean square velocity. Ar, CO2, Ne, O2 Answer 7: CO2 < Ar < O2 < Ne since larger molecules move slower than smaller molecules at the same T, place them in order by mass:
  • Click here👆to get an answer to your question ️ A gas bulb of 1 litre capacity contains 2.0 × 10^21 molecules of nitrogen exerting a pressure of 7.57 × 10^3 N m^-2 . Calculate the root mean square speed and temperature of the gas molecules. If the ratio of most probable speed to the root mean square speed is 0.82 , calculate the most probable speed of these molecules at this temperature.

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Calculate the root-mean-square speeds of helium atoms and nitrogen molecules in m/s at 25 o C. 7. The volume of oxygen collected at 24 o C and atmospheric pressure of 762 mmHg is 128 mL. Calculate the mass in grams of oxygen gas obtained. The pressure of the water vapor at 24 o C is 22.4 mmHg. 8.

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Assume that a certain sample of air maintained at 25 C contains dust particles all of which are the same size. The diameter of the dust particles is 5.0µm and their density is 2500 kg m−3. i. Find the most probable speed, the mean speed, and the root-mean-square speed of the dust particles, treating them as giant molecules. ii.

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(b) Air is a mixture of oxygen and nitrogen molecules. The mass of an oxygen molecule is greater than the mass of a nitrogen molecule. State and explain the effect this has on the mean square speeds of the oxygen and nitrogen molecules in the lungs. (3 marks) (Total 7 marks) Q6.

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Example Calculate the root-mean-square speed of oxygen molecules in air at 27 C. Solution The mass of a molecule of oxygen is 32.0 x1.66x10-27 kg, and the absolute temperature (T) = (273 + 27 = 300) K. Thus from Equation (3.12) we get 1 27 23 480 32.0 1.66 10 3 3 1.38 10 / 300 ms x x kg x x J Kx K m kT vrms

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Apr 25, 2013 · Calculate the root mean square velocity of nitrogen molecules at 25°C. 297 m/s 149 m/s 515 m/s 729 m/s

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If three molecules have velocities 0.5, 1 and 2 km/s respectively, calculate the ratio of the root mean square speed and average speed. At what temperature, will the root mean square velocity of a gas at 0 o C be half its value, if the pressure remains constant?

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