Which of the following gases of the same mass | vedclass

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(A) Let the mass of each gas be $m = 1 \ g$. The number of moles $n = \frac{m}{M}$,where $M$ is the molar mass. Since $m$ is constant,$n \propto \frac

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$H_2$

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(A) Let the mass of each gas be $m = 1 \ g$. The number of moles $n = \frac{m}{M}$,where $M$ is the molar mass. Since $m$ is constant,$n \propto \frac{1}{M}$. The molar masses are: $M(H_2) = 2 \ g/mol$,$M(N_2) = 28 \ g/mol$,$M(O_2) = 32 \ g/mol$,$M(Cl_2) = 71 \ g/mol$. Thus,the number of moles follows the order: $n(H_2) > n(N_2) > n(O_2) > n(Cl_2)$. From the ideal gas equation $PV = nRT$,at constant $T$ and $V$,$P \propto n$. Therefore,the gas with the highest number of moles will exert the highest pressure. Since $H_2$ has the lowest molar mass,it has the highest number of moles for a given mass,and thus exerts the highest pressure.

Which of the following gases of the same mass exerts the highest pressure at a constant temperature?

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