Assuming ideal gas behaviour,the ratio of den | vedclass

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(C) From the ideal gas equation,$PV = nRT$. Since $n = \frac{m}{M}$,we have $PV = \frac{mRT}{M}$. Rearranging for density $(d = \frac{m}{V})$,we get $

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$0.46$

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(C) From the ideal gas equation,$PV = nRT$. Since $n = \frac{m}{M}$,we have $PV = \frac{mRT}{M}$. Rearranging for density $(d = \frac{m}{V})$,we get $P = \frac{dRT}{M}$,which implies $d = \frac{PM}{RT}$. At constant temperature and pressure,$d \propto M$. Therefore,the ratio of densities is $\frac{d_{NH_3}}{d_{HCl}} = \frac{M_{NH_3}}{M_{HCl}}$. The molar mass of $NH_3 = 14 + 3(1) = 17 \ g/mol$. The molar mass of $HCl = 1 + 35.5 = 36.5 \ g/mol$. Ratio $= \frac{17}{36.5} \approx 0.4657 \approx 0.46$.

Assuming ideal gas behaviour,the ratio of density of ammonia to that of hydrogen chloride at the same temperature and pressure is: (Atomic wt. of $Cl = 35.5 \ u$)

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