Compute the average (root mean square) velocity (m/s) of Neon molecules at 356 Kelvins and 0.9 bars.

V = 20.6 m/s

Explanation:

Given that the temperature of the neon molecules = 356 Kelvin

Pressure = 0.9 bar

The mass number of Neon = 21.

Using the formula below

1/2 m v^2 = (3kT)/2

Where

T = temperature = 356 k

K = Bolzmann constant

= 1.38 × 10^-23jk^-1

NA = 6.02214076×10²³ mol⁻¹

Where NA = Avogadro number

Substitute all the parameters Into the formula

1/2 × 21/NA × v^2 = (3 × k × 356)/2

1.744×10^-23V^2 = 7.3692 × 10^-21

Make V^2 the subject of formula

V^2 = (7.37×10^-21)/1.744×10^-23

V^2 = 422.55

V = sqrt( 422.55)

V = 20.55

Therefore, the average (root mean square) velocity (m/s) of Neon molecules at 356 Kelvins and 0.9 bars is 20.55 m/s

answer:

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