Oxygen (molecular weight = 32) diffuses at a rate of 10cm3/min under the same conditions of temperature and pressure how fast will hydrogen (molecular weight = 2) diffuse ?
Correct answer: B. 40cm3/min
- A. 20cm3/min
- B. 40cm3/min
- C. 160cm3/min
- D. 2.5cm3/min
Explanation
Graham's law gives rate1/rate2 = √(M2/M1). Therefore, rate of hydrogen = 10 cm3/min x √(32/2) = 10 cm3/min x 4 = 40 cm3/min. The likely mistake is choosing 20 cm3/min by using the mass ratio directly instead of its square root.
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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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