Equal volumes of two monoatomic gases,$A$ and $B$ at same temperature and pressure are mixed. The ratio of specific heats $(C_P/C_V)$ of the mixture will be

Equal volumes of monoatomic and diatomic gases at same initial temperature and pressure are mixed. The ratio of specific heats of the mixture $({C_p}/{C_v})$ will be

At $300 \ K$ and $760 \ torr$ pressure, the density of a mixture of $He$ and $O_2$ gases is $0.543 \ g \ L^{-1}$. The mass percent of oxygen is approximately $(R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$

Which one of the following is the kinetic energy of a gaseous mixture containing $3 \ g$ of hydrogen and $80 \ g$ of oxygen at temperature $T(K)$ (in $RT$)?

If the density of a mixture of nitrogen and oxygen gases at $400 \ K$ and $1 \ atm$ pressure is $0.920 \ g \ L^{-1}$, what is the mole fraction of nitrogen in the mixture? ($R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$; assume ideal gas behavior for oxygen and nitrogen)

At $STP$,a closed vessel contains $1 \ mole$ each of $He$ and $CH_4$. Through a small hole,$2 \ L$ of $He$ and $1 \ L$ of $CH_4$ escaped from the vessel in '$t$' minutes. What are the mole fractions of $He$ and $CH_4$ respectively remaining in the vessel? (Assume $He$ and $CH_4$ as ideal gases. At $STP$,one mole of an ideal gas occupies $22.4 \ L$ of volume.)