wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Assume that you have a sample of a gas containing H2, HD and D2 that you want to separate into pure components (H= 1H and D= 2H). What are the relative rates of diffusion of the three gases according to Graham’s law?

A
H2>HD>D2
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
D2>HD>H2
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
D2>H2>HD
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
All have same rate
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A H2>HD>D2
According to Graham's law of diffusion,
Rate of diffusion=1Molar mass


Since D2 is the heaviest of the three molecules, it will be the slowest to diffuse and let us call its relative rate as 1.00. We can then compare the rate of diffusion of HD and H2 with D2 by using Graham's law of diffusion.

Comparing HD with D2 we have,
Rate of HD diffusionRate of D2 diffusion=Molar mass of D2Molar mass of HD=4.03.0=1.15

Comparing H2 with D2 we have,
Rate of H2 diffusionRate of D2 diffusion=Molar mass of D2Molar mass of H2=4.02.0=1.41

Thus, the relative rates of diffusion are H2(1.41)>HD(1.15)>D2(1.00)

flag
Suggest Corrections
thumbs-up
4
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Dalton's Law of Partial Pressure
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon