Dalton's Law of Partial Pressure

A gaseous mixture was prepared by taking equal mole of  $COand{N}_2.$ If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen  $(N_2)$ in the mixture is:

If 500ml of gas A at 400 torrs and 666.6 ml of B at 600 torrs are placed in a 3 liter flask, the pressure of the system will be

If 500ml of gas A at 400 torr and 666.6 ml of B at 600 torr are placed in a 3 litre flask, the pressure of the system will be

A gaseous mixture of $2$ moles of $\text{A}$, $3$ moles of $\text{B}$, $5$ moles of $\text{C}$ and $10$ moles of $\text{D}$ is contained in a vessel. Assuming that gases are ideal and the partial pressure of $\text{C}$ is $1.5$ atm, total pressure is

A cylinder was filled with gaseous mixture containing $\mathrm{CO}$ and ${\mathrm{N}}_2$ (equal masses). The ratio of their partial pressure in cylinder are

The partial pressure of a dry gas is

${\mathrm{p}}_{\mathrm{i}}={\mathrm{X}}_{\mathrm{i}}\times {\mathrm{P}}_{\mathrm{Total}}$

The above expression is related to 

A gaseous mixture was prepared by taking equal number of moles of Helium and Neon. If the total pressure of the mixture was found to be $10 \mathrm{atm},$ the partial pressure of Helium in the mixture is

A gaseous mixture contains $2$ moles of $\mathrm{A}, 3$ moles of $\mathrm{B}, 5$moles of $\mathrm{C}$ and $10$ moles of $\mathrm{D}$ contained in a vessel. If the gases are ideal and the partial pressure of $\mathrm{C}$ is $1.5 \mathrm{atm},$ then the partial pressure of $\mathrm{B}$ will be $\underline{ }$

If ${\mathrm{X}}_{\mathrm{M}}, {\mathrm{X}}_{\mathrm{P}}$ and ${\mathrm{X}}_{\mathrm{V}}$ are mole fraction, pressure fraction and volume fraction, respectively, of a gaseous mixture, then

A gaseous mixture contains three qases $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ with a total number of moles of $1.0$ and total pressure of $10$ atm. The partial pressure of $\mathrm{A}$ and $\mathrm{B}$ are $3$ atm and $1$ atm respectively and if $\mathrm{C}$ has molecular weight of $2 \mathrm{g}/\mathrm{mol}.$ Then, the weight of $\mathrm{C}$ present in the mixture will be :

A mixture of nitrogen and water vapour is admitted to a flask that contains a solid drying agent. Immediately after admission, the pressure in the flask is $760 \mathrm{Torr}$. After standing for some hours, the pressure reaches a steady value of $745 \mathrm{Torr}$. Calculate the mole percent of water vapour in the original mixture.

${\mathrm{O}}_2$ and ${\mathrm{SO}}_2$ gases are filled in ratio of $1 : 3$ by  moles in $6 \mathrm{L}$ (closed container) at temperature of $27°\mathrm{C}$. The partial pressure of ${\mathrm{O}}_2$ is $1.20 \mathrm{atm}$, the concentration of ${\mathrm{SO}}_2$ would be

A mixture of ${\mathrm{N}}_2$ and $\mathrm{Ar}$ gases in a cylinder contains $7\mathrm{g}$ of ${\mathrm{N}}_2$ and $8\mathrm{g}$ of $\mathrm{Ar}$. If the total pressure of the mixture of the gases in the cylinder is $27$ bar, the partial pressure of ${\mathrm{N}}_2$ is:
[Use atomic masses (in $\mathrm{g} {\mathrm{mol}}^{–1}$): $\mathrm{N}=14,\mathrm{Ar}=40$]

A mixture of helium and methane gases at $1.4$ bar pressure contains $20\%$ by mole of helium. The partial

pressure of helium will be :

The ratio of molar masses of ideal gases A and$B$ is$1: 4 .$ If pressure of a mixture containing equal mass of
$A$ and$B$ is$P$ $atm$, then the partial pressure of$B$ will be

A mixture of Neon and Ethane at $2 \mathrm{bar}$ pressure contains $20\%$ by mole of Neon. Partial pressure of Ethane will be:

Equal masses of sulphur dioxide and oxygen are mixed in an empty container at $25°\mathrm{C}$. The fraction of the total pressure exerted by sulphur dioxide is:

What will be the partial pressure of ${\mathrm{H}}_2$ in a flask containing $2 \mathrm{g}$ of ${\mathrm{H}}_2,14 \mathrm{g}$ of ${\mathrm{N}}_2$ and $16 \mathrm{g}$ of ${\mathrm{O}}_2$:

A gaseous mixture contains $56 \mathrm{g}$ of ${\mathrm{N}}_2, 44 \mathrm{g} {\mathrm{CO}}_2$ and $16 \mathrm{g}$ of ${\mathrm{CH}}_4$. The total pressure of the mixture is $720 \mathrm{mm}$ $\mathrm{Hg}$. The partial pressure of ${\mathrm{CH}}_4$ is: