Kinetic Molecular Theory and Gas Laws 2a) Use the kinetic molecular theory of ga

Question

Kinetic Molecular Theory and Gas Laws 2a) Use the kinetic molecular theory of gases to explain why gases are compressible? 2b) Carbon dioxide molecules have an average speed of 25.0 m/s at a given temperature and pressure. What is the average speed of carbon monoxide molecules at the same conditions.? 2c) Different amounts (by moles) of the same ideal gas are placed in separate flasks having the same volume and temperature. Using the KMT, compare (i) the density of the gases; (ii) the rms velocities of the gases; and (iii) the kinetic energies of the gases. Provide a brief justification for each answer

Explanation / Answer

a) Kinetic Molecular theory is based on various assumptions. One of the assumption is:

So since the gases have most of the empty space in between them they can be compressed.

b) For CO2, Molecular mass (M1) = 44g/mol

For CO, Molecular mass (M2) = 28 g/mol

We know, vrms = (3KBT/M)1/2

For CO2, vrms = (3KBT/M1)1/2

For CO let the velocity be v0 = (3KBT/M2)1/2

v0/vrms = (M1/M2)1/2

v0 = vrms(M1/M2)1/2

Putting values we get, v0 = 31.34 m/s

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