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

The $\%$ composition by volume of ${\mathrm{Cl}}_{2 },{\mathrm{N}}_2,{\mathrm{H}}_2$are in $1,2,7$ by proportion the total pressure is $40$ bar find the partial pressure of each gas

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?

Internal energy of $n_1$ mol of hydrogen of temperature $T$ is equal to the internal energy of $n_2$ mol of helium at temperature $2T$. The value of $\frac{10n_1}{n_2}$ is

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 $0.0821\mathrm{ }\times \mathrm{ }300=\mathrm{25]}$

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

A gaseous mixture containing $50 \mathrm{g}$ of nitrogen and $10 \mathrm{g}$ of oxygen were enclosed in a vessel of $10 \mathrm{L}$ capacity at ${27}^{\mathrm{o}}\mathrm{C}$. Calculate the partial pressure of each gas.

Density of a gas is found to be $5.46 \mathrm{g} /{\mathrm{dm}}^3$ at $300 \mathrm{K}$ and $2 \mathrm{bar}$ pressure. What will be its density at STP?

A large flask fitted with a stop-cock is evacuated and weighed; its mass is found to be$134.567 \mathrm{g}$. It is then filled to a pressure of $735 \mathrm{mm}$ at ${31}^{\mathrm{o}}\mathrm{C}$ with a gas of unknown molecular mass and then reweighed; its mass is $137.456 \mathrm{g}$.

The flask is then filled with water and weighed again; its mass is now $1067.9 \mathrm{g}$. Assuming that the gas is ideal, calculate the molar mass of the gas.