A container contains equal masses of H_2,He,C | vedclass

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(C) According to Dalton's Law of Partial Pressure,the partial pressure of a gas is directly proportional to its mole fraction $(x_i)$ in the mixture,i

Vedclass · Accepted Answer

$CO_2$

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(C) According to Dalton's Law of Partial Pressure,the partial pressure of a gas is directly proportional to its mole fraction $(x_i)$ in the mixture,i.e.,$P_i = x_i 	imes P_{total}$.Since $x_i = \frac{n_i}{n_{total}}$,the partial pressure is directly proportional to the number of moles $(n_i)$ of the gas.Given that the masses $(m)$ of all gases are equal,the number of moles is calculated as $n = \frac{m}{M}$,where $M$ is the molar mass.Thus,$n \propto \frac{1}{M}$.The molar masses are: $M(H_2) = 2 \ g/mol$,$M(He) = 4 \ g/mol$,$M(Ne) = 20 \ g/mol$,and $M(CO_2) = 44 \ g/mol$.Since $CO_2$ has the highest molar mass $(44 \ g/mol)$,it will have the minimum number of moles $(n = \frac{m}{44})$ for a fixed mass $m$.Therefore,$CO_2$ exerts the minimum partial pressure.

$A$ container contains equal masses of $H_2$,$He$,$CO_2$,and $Ne$ at a certain temperature. Which of the following gases exerts minimum partial pressure?

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