The graph drawn between pressure and volume in Boyle's law experiment is shown in figure for two different gases. If the same amount of both the gases has been taken, then the relationship between their molecular weights will be
M2<M1
M1<M2
M1=M2
M31=M2
A
M31=M2
B
M2<M1
C
M1<M2
D
M1=M2
Open in App
Solution
Verified by Toppr
From ideal gas equation, PV=nRT
And, n=wM where M is the molecular weight of the gas
Now, PV=wMRT
So, we draw a vertical line at a volume say V0.
Then for this volume, we see that pressure is higher for the gas with molecular weight M2 (from the graph) hence, this means that M2 must be smaller than M1.
Was this answer helpful?
2
Similar Questions
Q1
The graph drawn between pressure and volume in Boyle's law experiment is shown in figure for two different gases. If the same amount of both the gases has been taken, then the relationship between their molecular weights will be
View Solution
Q2
If the molecular weight of two gases are M1 and M2, then at a given tempreture the ratio of their root mean square velocity v1 and v2 will be