Derivation of Ideal Gas Equation MCQ - Practice Questions with Answers

Hydrogen bomb is based on the principle of

What is the density of $N_2$ gas at ${227}^{\circ }\mathrm{C}$ and 5.00 atm pressure? ( $\mathrm{R}=0.0821$ Latm $K^{-1}{\mathrm{mol}}^{-1}$ )

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 ]

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)

To an evacuated vessel with a Movable Piston under external pressure of 1 atm.
5 mole at He and 2 moles at  untrnoum compound [vapor pressure 68 atm at ${\mathrm{O}}^{\circ }\mathrm{C}$ ] is introduced considering the ideal Gas behavior.

The total volume (in lite) ot gas at $0^{\circ }\mathrm{C}$ is close to -

$\begin{array}{rl}& \text{ The Reduced Temperature }=\theta =\frac{\mathrm{T}}{{\mathrm{T}}_{\mathrm{A}}}\\ & \text{ The Reduced Pressure }=\mathrm{\Gamma }=\frac{\mathrm{P}}{{\mathrm{P}}_{\mathrm{A}}}\\ & \text{ The Reduced volume }=\varphi =\frac{\mathrm{V}}{{\mathrm{V}}_{\mathrm{A}}}\end{array}$

Hence, it can be said that the Reduced equation of state may be given as 

Two glass bulbs A and B are connected by a very Small Tube having a stop-cock. Bulb A has a volume $50{\mathrm{cm}}^3$ and contained the gas, mutule bulb B was empty. On opening the stop-cocts. the pressure fall down to $50\mathrm{\%}$ The volume at bulb B must be

A $5.0L$ elast contains 32 g at oxygen at ${27}^{\circ }\mathrm{C}$ [Assume ${\mathrm{O}}_2$ is betwaing ideally] The pressure involev the elask in bar is[Given $\mathrm{R}=.0831{\mathrm{L}}_{\text{bar }}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$ ]

Choose the correct option for the total bossing in a mixture of $6{\mathrm{gO}}_2$ and $4{\mathrm{gH}}_2$ confined in a total volume of one litre at ${\mathrm{O}}^{\circ }\mathrm{C}$ is ?

${}_{[}\mathrm{R}=082\mathrm{Latm}{\mathrm{mol}}^{-1}{\mathrm{H}}^{-1},\mathrm{T}=273{\mathrm{k}}_{]}$
 

The volume occupied by$g\mathrm{g}$ of water vapour at ${300}^{\circ }\mathrm{C}$ and 1 bar pressure will be
[$\mathrm{R}=.083{\mathrm{bar}{\mathrm{Lk}}^{-1}{\mathrm{mol}}^{-1}}^{-1}$]