A) \[\frac{2}{3}\]
B) \[\frac{3}{4}\]
C) \[2\]
D) \[\frac{1}{2}\]
Correct Answer: B
Solution :
\[{{\rho }_{A}}=1.5{{\rho }_{B}}\] \[{{\rho }_{B}}\] \[{{\rho }_{A}}=2{{\rho }_{B}}\] \[{{p}_{B}}\] According to ideal gas equation, we have Pressure,\[p=\frac{\rho RT}{M}\], where M is molecular weight of ideal gas. Such that, \[\frac{p}{\rho }=\frac{RT}{M}\Rightarrow M=\frac{\rho RT}{p}\] where, R and T are constant. So, \[M\propto \frac{\rho }{p}\] \[\Rightarrow \,\,\frac{{{M}_{A}}}{{{M}_{B}}}=\frac{{{\rho }_{A}}}{{{\rho }_{B}}}\times \frac{{{p}_{B}}}{{{p}_{A}}}=1.5\times \frac{1}{2}=0.75=\frac{3}{4}\]You need to login to perform this action.
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