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 contain hydrogen and nitrogen. The mole fraction of ${\mathrm{H}}_2$ in the gaseous mixture is $0.6$. If the pressure of the gaseous mixture is $2.8 \mathrm{atm}$. Calculate the partial pressures of ${\mathrm{H}}_2$ and ${\mathrm{N}}_2$ in the mixture.

$400\mathrm{ml} \mathrm{of} \mathrm{He}$ gas at 4 atm is mixed with 600 ml of Ne Gas at 3 atm, in vessel of $5.0\mathrm{L}$ capacity. Calculate the partial pressure and total pressure of gaseous mixture.

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

One litre of water is kept in a closed two litre vessel at temperature $\mathrm{T}$ with no air in the space above the liquid (System $1$). Another identical system is prepared but there is air above the liquid (System $2$). Assuming water vapour as well as air to behave as ideal gases and water to be in equilibrium with the vapour above the liquid, the correct statement(s) is/are

Explain Dalton's law of partial pressure of gases.

Two flasks of capacity $1 \mathrm{L}$ and $2 \mathrm{L}$ contain gases, $\mathrm{A}$ and $\mathrm{B}$ respectively at same temperature. If density of $\mathrm{A}$ is $2.5 \mathrm{g}/\mathrm{L}$ and that of $\mathrm{B}$ is $5 \mathrm{g}/\mathrm{L}$ and the molar mass of $\mathrm{A}$ is twice of that of $\mathrm{B}$, then the ratio of pressure exerted by gases $\left(\mathrm{A}:\mathrm{B}\right)$ is

A mixture of ${\mathrm{N}}_2$ and ${\mathrm{CO}}_2$ at one atm pressure contains $56\%$ by weight of ${\mathrm{N}}_2$. Partial pressure of ${\mathrm{N}}_2$ in the mixture will be

Which mixture of gases at room temperature does not obey Dalton's law of partial pressure?

$2 \mathrm{g}$ of gas $\mathrm{A}$ introduced in a evacuated flask at $25°\mathrm{C}$. The pressure of the gas is $1 \mathrm{atm}$. Now $3 \mathrm{g}$ of another gas $\mathrm{B}$ is introduced in the same flask so total pressure becomes $1.5 \mathrm{atm}$. The ratio of molecular mass of $\mathrm{A}$ and $\mathrm{B}$ is

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 

The total pressure exerted by the mixture of non-reactive gases is equal to the sum of the _____ pressures of individual gases.

Define and derive the Dalton’s law of partial pressures.

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 $\underline{ }$

Oxygen and cyclopropane at partial pressure of 570 torr and 170 torr respectively are mixed in a gas cylinder. The ratio of the number of moles of cyclopropane to the number of moles of oxygen is:

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 :