If he (g) has an average kinetic energy of 5610 j/mol under certain conditions, what is the root mean square speed of o2 (g) molecules under the same conditions?

Kinetic energy is the energy possessed by a particle or a body when in motion.

It is calculated by 1/2 mv², where m is the mass and v is the velocity.

But from the Grahams law of diffusion

V (he) / V (o2) = √ (M (o2) / M (he)

= √ (32/4)

= 2.83

This means that Helium diffuses at a rate of 2.83 times faster than oxygen.

Since the conditions are the same then the two gases will have equal kinetic energy,

Hence; (He = 4g/mol, O2 = 32g/mol

5610 = 0.5 * 4/1000 * v²

v² = 2805000

v = 1674.8 m/s for He

Therefore, since He diffuses at a rate of 2.83 times faster than oxygen

Then, the velocity of Oxygen will be;

1674.8/2.83

= 591.8 m/s

Thus, the velocity of oxygen molecules is 591.8 m/s