Ideal Gas Equation

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

Cyclopropane and oxygen at partial pressures $170$ torr and $570$ 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  $\left(\frac{{\mathrm{nC}}_3{\mathrm{H}}_6}{{\mathrm{nO}}_2}\right)?$ (Assume no reaction).

If $\mathrm{P}, \mathrm{V}, \mathrm{M}, \mathrm{T} \mathrm{and} \mathrm{R}$ are pressure, volume, molar mass, temperature and gas constant respectively, then for an ideal gas, the density is given by

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

The density of the gaseous mixture in a vessel $\left({\mathrm{N}}_2\mathrm{ }\mathrm{and}\mathrm{ }\mathrm{He}\right)$ at 2.1 atmosphere and 310 K is 1.35 g/litre. If a small pin-hole is made on the wall of the vessel, through which gases effuse, then which of the following is the correct composition of the gases He and ${\mathrm{N}}_2$   effusing out initially?

Calculate the number of hours (up to the nearest integer) of service that can be derived at $1 \mathrm{atm}$, $\mathrm{300 }\mathrm{K}$ from an acetylene lamp containing $640\mathrm{ }\mathrm{g}$ calcium carbide. Given that the lamp requires $50\mathrm{ }\mathrm{L}$ acetylene gas at $1 \mathrm{atm}$, $\mathrm{300 }\mathrm{K}$ for one hour. [Take $0.0821\mathrm{ }\times \mathrm{ }300=\mathrm{25]}$

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

Give relationship pressure exerted by the gas and its mole fraction of the mixture.

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

If $4$ moles of an ideal gas at $300 \mathrm{K}$ occupies volume of $89.6 \mathrm{L}$, then pressure of the gas will be _____$\mathrm{atm}$.(write with four significant figures)

Calculate the number of hours (up to nearest integer)  of service that can be derived at 1 atm, $\mathrm{300 }\mathrm{K}$ from an acetylene lamp containing $640\mathrm{ }\mathrm{g}$ calcium carbide. Given that the lamp requires $50\mathrm{ }\mathrm{L}$ acetylene gas at 1 atm $\mathrm{300 }\mathrm{K}$ for one hour. [Take $0.0821\mathrm{ }\times \mathrm{ }300=\mathrm{25]}$

Calculate the number of hours of service that can be derived at 1 atm, $\mathrm{300 }\mathrm{K}$ from an acetylene lamp containing $640\mathrm{ }\mathrm{g}$ calcium carbide. Given that the lamp requires $50\mathrm{ }\mathrm{L}$ acetylene gas at 1 atm $\mathrm{300 }\mathrm{K}$ for one hour. [Take $0.0821\mathrm{ }\times \mathrm{ }300=\mathrm{25]}$

The pressure of a mixture of '$\mathrm{x}$' gram of oxygen gas and $1$ mole of hydrogen gas contained in a vessel of $1 \mathrm{litre}$ at $0°\mathrm{C}$ is $25.215 \mathrm{atm}$. The value of '$\mathrm{x}$' is:

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

Which one of the following schematic graphs best represents the variation of $p V$ (in Joules) versus $T$ (in Kelvin) of one mole of an ideal gas? (The dotted line represents $p V=T$ )

A container of volume $2.24 \text{L}$can with stand a maximum pressure of $2$ atm at $298 \text{K}$ before exploding. The maximum amount of nitrogen (in $\text{g}$) that can be safely put in this container at this temperature is closest to

$16 \mathrm{g}$ 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.