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# To which of the following the Dalton’s law of partial pressure is not applicable?A) ${H_2}$ and $He$B) $N{H_3}$ and $HCl$C) ${N_2}$ and ${H_2}$D) ${N_2}$ and ${O_2}$

Last updated date: 17th Jun 2024
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Hint: Dalton's law of partial pressures states that the total pressure of a gas mixture is the summation of partial pressures of its components. It can be given as,
${{\rm{P}}_{\rm{T}}} = {{\rm{P}}_{\rm{1}}} + {{\rm{P}}_{\rm{2}}} + {{\rm{P}}_3} + ........$
Here, ${{\rm{P}}_{\rm{T}}}$implies the total pressure of the gas and ${{\rm{P}}_2}$, ${{\rm{P}}_2}$ and ${{\rm{P}}_3}$are the partial pressures of its components 1, 2,3 etc.

Dalton's law of partial pressure is applicable when the component of the gases in a mixture does not react with each other. It is also not applicable when the mixture of reacting gases is at room temperature for. Dalton's law of partial pressure is not applicable when a gas reacts under experimental conditions. As the $N{H_3}$ and $HCl$ reacts under the ordinary conditions, Dalton's law of partial pressure is not applicable to this mixture.
${{\rm{X}}_{\rm{i}}} = {{\rm{P}}_{\rm{i}}}{{\rm{P}}_{{\rm{total}}}} = {{\rm{V}}_{\rm{i}}}{{\rm{V}}_{{\rm{total}}}} = {{\rm{n}}_{\rm{i}}}{{\rm{n}}_{{\rm{total}}}}$
Here,${{\rm{X}}_{\rm{i}}}$ is the mole fraction of a gas ‘${\rm{i}}$’ in a mixture of ‘${\rm{n}}$’ gases, ‘${\rm{n}}$’ is the number of moles, ‘${\rm{P}}$is the pressure, and ${\rm{V}}$ denotes volume.