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

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Question

(A) According to Dalton's Law of partial pressure,the partial pressure of a gas is directly proportional to its mole fraction $(P_i = X_i P_{total})$.

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$H_2$

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(A) According to Dalton's Law of partial pressure,the partial pressure of a gas is directly proportional to its mole fraction $(P_i = X_i P_{total})$.Since the temperature and volume are constant,the mole fraction $X_i$ is proportional to the number of moles $n_i$.Let the mass of each gas be $m$.The number of moles $n_i$ is given by $n_i = \frac{m}{M_i}$,where $M_i$ is the molar mass.For $H_2$: $n = \frac{m}{2}$For $He$: $n = \frac{m}{4}$For $CO_2$: $n = \frac{m}{44}$For $Ne$: $n = \frac{m}{20}$Comparing the number of moles,the gas with the smallest molar mass will have the highest number of moles.Since $H_2$ has the smallest molar mass $(2 \ g/mol)$,it will have the maximum number of moles and therefore exert the maximum partial pressure.

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

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