Consider neon, a noble gas whose molecules consist of single atoms of atomic mass 0.02 kg/mol. what is the average kinetic energy of a neon atom when the gas is at a temperature of 370 k? avogadro’s number is 6.02 × 1023 mol−1 and boltzmann’s constant is 1.38 × 10−23 j/k. answer in units of j. question 5, chap 19, sect 4. part 2 of 3 10 points what is the root mean square speed of a neon atom under such conditions? answer in units of m/s.

Answer :

The average kinetic energy is,

The root mean square speed is,

Explanation:

(a) The formula for average kinetic energy is:

where,

k = Boltzmann’s constant =

T = temperature = 370 K

Now put all the given values in the above average kinetic energy formula, we get:

The average kinetic energy is,

(b) The formula used for root mean square speed is:

where,

= root mean square speed

k = Boltzmann’s constant =

T = temperature = 370 K

M = atomic mass = 0.02 kg/mole

= Avogadro’s number =

Now put all the given values in the above root mean square speed formula, we get:

The root mean square speed is,

i think it is true since you can test the answer and can use observations to complete it.