Derivation of Ideal Gas Equation - Practice Questions & MCQ

An open vessel at $27^{\circ} \mathrm{C}$ is heated until two fifth of the air (assumed as an ideal gas ) in it has escaped from the vessel. Assuming that the volume of the vessel remains constant, the temperature at which the vessel has been heated is: (in K)

Hydrogen bomb is based on the principle of

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of 1 atm but also a concentration of  1 mol litre^-1.   [ R = 0.082 litre atm mol^-1 K^-1 ]

The behavior of a real g is usually depicted by plotting compressibility factor z versus p at a constant temperature This fact can be explained by the van der Wads equation when -
 

 An open vessel at $27^{\circ} \mathrm{C}$ is heated until two fifth of the ain in it has escaped from the vessel. Assuming that the volume of the Vessel remains constant, the temperature at which the vessel has been heard in -

The density of neon will be highest at -

At $0^{\circ} \mathrm{C}$, the density of a gaseous oxide at 2 bar is same as that of nitrogen at 5 bar. What is the molecular mass of the oxide?

A 21 flask contains $0.4 \mathrm{~g} \mathrm{O}_2$ and $0.6 \mathrm{~g} \mathrm{H}_2 100^{\circ} \mathrm{C}$. Calculate the total pressure of the gas mixture in the flask. $\qquad$

At , the density of a certain oxide of a gas at bars is the same as that of dinitrogen at 5 bars. what is the molecular mass of the oxide ________?

Pressure of 1 g of an ideal gas A at $27^{\circ} \mathrm{C}$ is found to be 2 bar. when 2 g of another ideal gas B is introduced in the same flask at same temperature, the pressure becomes 3 bar. Find a relationship between their molecular masses $\qquad$.