A gas diffuses 1/2 times as fast as hydrogen, its molecular mass is:
Correct answer: D. 8 amu
- A. 50 amu
- B. 25 amu
- C. 16 amu
- D. 8 amu
Explanation
Graham found experimentally that the rate of diffusion of a gas is inversely proportional to the square root of the mass of its particles. v1/v2=√(M2/M1) where M1=H2 v1/(1/2)v1 =√(M2/2) 2²=M2/2 => M2 = 4×2 = 8
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About Kinetic Molecular Theory
Kinetic molecular theory explains gases as rapidly moving particles separated by large distances, with negligible volume and negligible intermolecular attraction in the ideal model. It relates temperature to average kinetic energy and explains gas pressure, Boyle's and Charles's laws, diffusion, effusion and the conditions under which real gases deviate from ideal behavior.
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