1.Plot the Maxwell-Boltzmann distribution function, p(v), for molecular speeds v
ID: 546999 • Letter: 1
Question
1.Plot the Maxwell-Boltzmann distribution function, p(v), for molecular speeds versus the speed, v, for N2 gas at -100.0°C and 1400° C. Locate the most probable speed, the average speed, and the root mean square speed on both graphs. Turn in the graphs, the spread sheets, and the typed spreadsheet formulas for each column-no two students should have exactly the same spreadsheet formats. 2 what is the mean relative velocity at 300 K for nitrogen and oxygen molecules. 3. A vessel contains 02 at 8.0 torr pressure and a temperature of 250.0 K. Assuming a molecular diameter of 0.295 nm, how many O2-02 collisions will occur per cm per second?Explanation / Answer
Answer:
Mean Relative velocity i.e RMS velocity is given as
v = [3RT/M]1/2.
Where R = Molar gas constant = 8.314 J/mole.K, T = 300 K, M = Molar mass in Kg/mole.
i) For N2 molecule, M = 28 g/mole = 0.028 Kg/mole.
using these values in above equation,
v = [3 x (8.314 J/mmole.K) x (300 K) / (0.028 Kg/mole)]1/2
v = 516.95 m/s.
ii) For O2 molecule.
Molar mass of O2 = 32 g/mole = 0.032 Kg/mole.
Using above formula again we get,
v = [3 x (8.314 J/mmole.K) x (300 K) / (0.032 Kg/mole)]1/2.
v = 483.56 m/s.
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