Which one of the following gas has the highest rate of diffusion at the same temperature and pressure?
Correct answer: C. C2H2
- A. HCL
- B. CO2
- C. C2H2
- D. C2H6
Explanation
Graham Law states Rate of Diffusion ∝ 1/√(MolecularMass) Option A: HCl has molecular mass 36g Option B: CO2 has molecular mass 44g Option C: C2H2 has molecular mass 26g Option D: C2H6 has molecular mass 30g As C2H2 has lowest molecular mass, it has highest rate of diffusion.
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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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