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 mixture of ${\mathrm{H}}_2\mathrm{O} ,{\mathrm{CO}}_2$​ and ${\mathrm{N}}_2$​ are trapped in a glass apparatus with a volume of $0.731 \mathrm{mL}$. The pressure of total mixture was $1.74\mathrm{mm}$ of Hg at $23°\mathrm{C}$. The sample was transferred to a bulb in contact with dry ice($-75°\mathrm{C}$) so that $\mathrm{H}2\mathrm{O}\left(\mathrm{v}\right)$ are frozen out. When the sample returned to the normal value of temperature, the pressure was $1.32\mathrm{mm}$ of Hg. The sample was then transferred to bulb in contact with liquid ${\mathrm{N}}_2(-75°\mathrm{C})$ to freeze out ${\mathrm{CO}}_2$​. In the measured volume, the pressure was $0.53\mathrm{mm}$ of Hg at original temperature. Mole of ${\mathrm{N}}_2$​ in mixture are $2.1\times {10}^{-\mathrm{y}}$.
So, the value of $\mathrm{y}$ is......(as nearest integer)

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

Which one is not correct mathematical equation for Dalton's Law of partial pressure? Here $\mathrm{P}=$ total pressure of gaseous mixture

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

$16 \mathrm{g}$ each of ${\mathrm{H}}_2$, $\mathrm{He}$ and ${\mathrm{O}}_2$ are present in a container exerting $10 \mathrm{atm}$ pressure at $\mathrm{T}\left(\mathrm{K}\right)$. The pressure in atm exerted by$16 \mathrm{g}$ each of $\mathrm{He}$ and ${\mathrm{O}}_2$ in the second container of same volume and temperature is

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.

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 $\mathrm{g} {\mathrm{mol}}^{–1}$): $\mathrm{N}=14,\mathrm{Ar}=40$]

Dehumidifier is used to reduce the humidity of air. In the following figure a dehumidifier is shown.

At $400\mathrm{K}$, saturation vapour pressure $=0.06\mathrm{atm}$.
At $300\mathrm{K}$, saturation vapour pressure $=0.04\mathrm{atm}$.
If the above dehumidifier is operated for $1$ hour how many gram of water will be collected from dehumidifier in nearest possible integer?

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

Calculate partial pressure (in bar) of ${\mathrm{O}}_2$, if the density of a mixture of ${\mathrm{O}}_2$ and ${\mathrm{N}}_2$ is $1.3\mathrm{ }{\mathrm{gL}}^{-1}$ at STP.

A mixture contains equal masses of ${\mathrm{H}}_2, {\mathrm{O}}_2 \mathrm{and} {\mathrm{CH}}_4$ gas at a total pressure of $380$ torr. The partial pressure of ${\mathrm{CH}}_4$ is

Total pressure is $2.1 \mathrm{atm}$ and equal masses of ${\mathrm{SO}}_2$, ${\mathrm{CH}}_4$ and ${\mathrm{O}}_2$ are mixed in an empty container at $298 \mathrm{K}$. Calculate the partial pressure of ${\mathrm{CH}}_4$ in the mixture. (Assume non reacting mixture)

The total pressure of sample of air containing only ${\mathrm{N}}_2,\mathrm{ }{\mathrm{H}}_2$ and saturated with water vapours is 640 torr. The aqueous tension of water is 40 torr and the molar ratio of ${\mathrm{N}}_2\mathrm{ }:{\mathrm{H}}_2$ is 3 : 1. The partial pressure of ${\mathrm{N}}_2$ in the sample is? (Assume there is no reaction taking place between nitrogen and hydrogen).

In the reaction, ${\mathrm{N}}_2+3{\mathrm{H}}_2\to 2{\mathrm{NH}}_3$ initially, we take  $2 \mathrm{mol}$ of ${\mathrm{N}}_2$ and $5 \mathrm{mol}$ of ${\mathrm{H}}_2$ exerting a total pressure of $7 \mathrm{atm}$ at a given temperature in a closed vessel. When $50\mathrm{\%}$ of ${\mathrm{N}}_2$ is converted into ${\mathrm{NH}}_3$, the partial pressure of $\mathrm{N}{\mathrm{H}}_3$ would be?

In which of the following mixtures, Dalton's law of partial pressure is not applicable? (Assume room temperature)

The total pressure of a mixture of ${\mathrm{H}}_2$ and ${\mathrm{O}}_2$ is 1.00 bar. Water, which is formed due to reaction between ${\mathrm{H}}_2$ and ${\mathrm{O}}_2$, is completely removed in the form of liquid to leave pure stains of ${\mathrm{H}}_2$ at a pressure of 0.35 bar. Assuming ideal gas behavior and all pressure measurements were made under the same conditions of temperature and volume, what is the mole fraction of ${\mathrm{H}}_2$ in the original mixture?