25 g of each of the following gases are take | vedclass

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(C) According to the ideal gas equation,$PV = nRT$,where $n = \frac{m}{M}$.Since $P$,$V$,$T$,and $m$ are given,$V = \frac{mRT}{PM}$.For a fixed mass $

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$HI$

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(C) According to the ideal gas equation,$PV = nRT$,where $n = \frac{m}{M}$.Since $P$,$V$,$T$,and $m$ are given,$V = \frac{mRT}{PM}$.For a fixed mass $(m = 25 \ g)$,temperature $(T)$,and pressure $(P)$,the volume $V$ is inversely proportional to the molar mass $M$ $(V \propto \frac{1}{M})$.The molar masses of the gases are: $M(HF) = 20 \ g/mol$,$M(HCl) = 36.5 \ g/mol$,$M(HBr) = 81 \ g/mol$,and $M(HI) = 128 \ g/mol$.Since $HI$ has the highest molar mass,it will have the least number of moles and consequently the least volume.

$25 \ g$ of each of the following gases are taken at $27^{\circ}C$ and $600 \ mm$ pressure. Which of these will have the least volume?

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