Average kinetic energy gas problem?

Question

A 5.00 L flask is filled with a sample of fluorine at a temp of 301.8 C. Calculate the average kinetic energy and rms speed in SI units.

Answer 1

Use the formulas
Kinetic Energy = (3/2) k T = M v^2 /(2N)
where
T is temperature in Kelvin
M is molar mass
N is Avogadro's constant
k =R/N is Boltzman constant

1) Average kinetic energy
K.E. = (3/2) 8.3145 J/(mol K) * (301.8+273.2) K = 7171 J/mol

2) rms speed
u = sqrt(3k N T / M)
= sqrt(3 R T / M)
= sqrt(3*8.3145*575 / 0.019)
= 869 m/s
Note that I took M=0.019 kg/mol as the molar mass

There is more help on this kind of problems here:
http://www.science.uwaterloo.ca/~cchieh/cact/c120/gaskinetics.html

Answer 2

Use Ideal gas law to solve for number of moles of fluorine gas. Change Celsius to Kelvin

I don't remember the formula for ave. kin. E and speed, but the only things that gases depend on are temp and #moles. Look up R value for your particular units.

Answer 3

Use perfect gas regulation to unravel for type of moles of fluorine gas. commerce Celsius to Kelvin i do not think concerning the elements for ave. relations contributors. E and %, although the only concerns that gases matter upon are temp and #moles. seem up R well worth on your diverse fashions.