Confused about ideal gas law with two types of gases Suppose I have a ideal gas mixture consisting of two different types of ideal gases, say $A$ and $B$, in a container with volume $V_{tot}$. There are $N_A$ particles of gas $A$ and $N_B$ particles of gas $B$. The temperature and pressure of the mixture are denotes by $T$ and $P$. Can I still use the ideal gas law for each of the component? Take $A$ as an example, is the following true?
$$P_A=\rho_A \frac{R}{M_A}T,$$ and
$$V_{\text{m},A}=\frac{V_{tot}}{N_A}=\frac{RT}{P_A}=\frac{M_A}{\rho_A}$$
where $P_\text{A}$ is the partial pressure, $M_A$ is the molar mass, $V_{\text{m},A}$ is the partial molar volume, and $\rho_A$ is the partial density of $A$, i.e., the mass of species $A$ per unit volume of the mixture gas. $R$ is the universal gas constant. Thanks a lot!
 A: Remember that ideal gases do not interact. They don't interact with themselves or with other ideal gases, so in a mixture of ideal gases each component of the mixture behaves as if the other gases were not present.
So for every type of gas present the ideal gas equation holds:
$$ P_i = n_i\frac{RT}{V} \tag{1} $$
And the total pressure is just the sum of all these partial pressures:
$$ P_{tot} = \sum_i P_i = \sum_i n_i\frac{RT}{V} \tag{2} $$
This can be rewritten in various ways using:
$$ \rho_i = \frac{M_i n_i}{V} $$
where $M_i$ is the molecular weight of the gas $i$, so $M_i n_i$ is the total mass present of species $i$. For example we can rewrite this as:
$$ \frac{V\rho_i}{M_i} = n_i $$
and susbtitute this into equation (1) to get the equation you give:
$$ P_i = n_i\frac{RT}{V} = \frac{V\rho_i}{M_i}\frac{RT}{V} = \frac{\rho_i}{M_i}RT $$
However it isn't useful to talk about a partial molar volume as all the gas molecules are uniformly distributed. It would only make sense to talk about $V_i$ if the two gases were separated by a movable partition so they were at the same temperature and pressure but had different volumes:

