Dalton's Law of Partial Pressure

The density of a mixture of ${\mathrm{O}}_2$ and ${\mathrm{N}}_2$ at NTP is $1.3 \mathrm{g} {\mathrm{litre}}^{-1}$. Calculate the partial pressure of ${\mathrm{O}}_2$.

The mass of the molecule $\mathrm{A}$ is twice that of the molecule $\mathrm{B}$. The root-mean-square velocity of the molecule $\mathrm{A}$ is twice that of the molecule $\mathrm{B}$. If two containers of equal volumes have the same number of molecules, the ratio of the pressures ${\mathrm{P}}_{\mathrm{A}}/{\mathrm{P}}_{\mathrm{B}}$ will be

The partial pressure of hydrogen in a flask containing two grams of hydrogen and $32 \mathrm{gm}$ of sulphur dioxide is

The partial pressure of hydrogen in a flask, containing two grams of hydrogen and $32 \mathrm{g}$ of sulphur dioxide, is

Oxygen and cyclopropane at partial pressures of $570 \mathrm{torr}$ and $170 \mathrm{torr}$, respectively, are mixed in a gas cylinder. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen?

Equal weights of ethane and hydrogen are mixed in an empty container at $25°\mathrm{C}$, the fraction of the total pressure exerted by hydrogen is

A $0.5 {\mathrm{dm}}^3$ flask contains the gas $\mathrm{A}$, and a $1 {\mathrm{dm}}^3$ flask contains the gas $\mathrm{B}$ at the same temperature. If the density of $\mathrm{A}=3 \mathrm{g}/{\mathrm{dm}}^3$ and that of $\mathrm{B}=1.5 \mathrm{g}/{\mathrm{dm}}^3$, and the molar mass of $\mathrm{A}=1/2$ of $\mathrm{B}$, the ratio of the pressure exerted by the gases is