1.Plot the Maxwell-Boltzmann distribution function, p(v), for molecular speeds v

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

3. Pressure of Oxygen gas = 8 torr = 0.01052 atm

Temperature = 250 K

Volume = 1 cu. cm = 0.001 litres

R= 0.0821 litre.atm/mol K

Using ideal gas equation, n= PV/RT

Thus number of moles of Oxygen gas = 5.131 * 10^-7 moles.

1 mole of gas consists of 6.023*10^23 moles (Avogadro's Number)

Thus number of molecules present = 30.904 * 10^16 molecules

Diameter of oxygen molecule = 0.295 nm = 0.295 * 10^-7 cm

Thus C/S area = (3.14/4) * (0.295 *10^-7)^2 = 0.0683 * 10^-14 = 6.83*10^-16 cm2

Number density = No of particles/ Volume = 3.0904 * 10^17 molecules/ cu. cm

Thus number of collisions per second = 3.0904*10^17* 6.83*10^-16 = 211 collisions per second

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