Five grams each of the following gases at 87 | vedclass

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(D) According to the ideal gas equation,$PV = nRT$,where $n = \frac{w}{M}$.Substituting $n$,we get $PV = \frac{w}{M} RT$,which implies $V = \frac{wRT}

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$HI$

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(D) According to the ideal gas equation,$PV = nRT$,where $n = \frac{w}{M}$.Substituting $n$,we get $PV = \frac{w}{M} RT$,which implies $V = \frac{wRT}{PM}$.Since $w$,$R$,$T$,and $P$ are constant for all gases,the volume $V$ is inversely proportional to the molar mass $M$ $(V \propto \frac{1}{M})$.Therefore,the gas with the highest molar mass will have the least volume.The molar masses are: $HF = 20 \, g/mol$,$HCl = 36.5 \, g/mol$,$HBr = 81 \, g/mol$,and $HI = 128 \, g/mol$.Since $HI$ has the highest molar mass,it will occupy the least volume.

Five grams each of the following gases at $87 \, ^{\circ}C$ and $750 \, mm$ pressure are taken. Which of them will have the least volume?

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