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I am currently studying Atkins' Physical Chemistry, 11th edition, by Peter Atkins, Julio de Paula, and James Keeler. Chapter 1A.2 Equations of state says the following:

When dealing with gaseous mixtures, it is often necessary to know the contribution that each component makes to the total pressure of the sample. The partial pressure, $p_J$, of a gas $J$ in a mixture (any gas, not just a perfect gas), is defined $$p_J = x_J p \tag{1A.6}$$ where $x_J$ is the mole fraction of the component $J$, the amount of $J$ expressed as a fraction of the total amount of molecules, $n$, in the sample: $$x_J = \dfrac{n_J}{n} \ \ \ n = n_A + n_B + \dots \tag{1A.7}$$ When no $J$ molecules are present, $x_J = 0$; when only $J$ molecules are present, $x_J = 1$. It follows from the definition of $x_J$ that, whatever the composition of the mixture, $x_A + x_B + \dots = 1$ and therefore that the sum of the partial pressures is equal to the total pressure: $$p_A + p_B + \dots = (x_A + x_B + \dots)p = p \tag{1A.8}$$ This relation is true for both real and perfect gases.

When all the gases are perfect, the partial pressure as defined in eqn 1A.6 is also the pressure that each gas would exert if it occupied the same container alone at the same temperature.

It is this last part that I am unsure about:

When all the gases are perfect, the partial pressure as defined in eqn 1A.6 is also the pressure that each gas would exert if it occupied the same container alone at the same temperature.

I don't understand why this is true. Furthermore, is this not in reference to the perfect gas law, $pV = nRT$? Then how does this relate to $pV = nRT$?

I would greatly appreciate it if people would please take the time to clarify this.

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  • $\begingroup$ Well, if $p_{total}V=n_{total}RT$, and $n_A=n_{total}\cdot x_A$, then what is $p_A$? $\endgroup$
    – Ivan Neretin
    Jun 16 '20 at 5:49
  • $\begingroup$ @IvanNeretin So $p_A = x_A p_{\text{total}} \Rightarrow p_{\text{total}} = \dfrac{p_A}{x_A}$ by 1A.6, and so we have that $\dfrac{p_A}{x_A} V = n_{\text{total}} RT$? $\endgroup$
    – The Pointer
    Jun 18 '20 at 9:30
  • $\begingroup$ @IvanNeretin And what about the other part of the question? Why is it that, when all the gases are perfect, the partial pressure as defined in eqn 1A.6 is also the pressure that each gas would exert if it occupied the same container alone at the same temperature? $\endgroup$
    – The Pointer
    Jun 18 '20 at 9:32
  • $\begingroup$ Why is it that if $2a=4$ then $a=2$? That's how algebra works. $\endgroup$
    – Ivan Neretin
    Jun 18 '20 at 9:40
  • $\begingroup$ @IvanNeretin I mean the qualitative explanation. $\endgroup$
    – The Pointer
    Jun 18 '20 at 9:41
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Partial pressure is defined as the pressure a component of a gaseous mixture would exert if it alone were to occupy the container at the same temperature as that of the mixture.

If the gases in the mixture are ideal, you can apply the ideal gas equation for it $$p_A V = n_ART$$where $p_A$ and $n_A$ represents the partial pressure and number of moles of a component A. Also $$p_tV = nRT$$ where $p_t$ and $n$ represents the total pressure and number of moles of the gaseous mixture. Dividing these equations you will get $$\frac{p_A}{p_t}=x_A$$ This equation will only be true for ideal gas mixture.

Also, partial pressure is a notional concept. It is not a the actual pressure exerted by the components. It was introduced to explain and form physical properties of gaseous mixtures.

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