The pressure exerted by a non-reactive gaseous mixture of $6.4 \ g$ of methane and $8.8 \ g$ of carbon dioxide in a $10 \ L$ vessel at $27^{\circ} C$ is .............$kPa$.
(Round off to the Nearest Integer).
[Assume gases are ideal,$R = 8.314 \ J \ mol^{-1} K^{-1}$
Atomic masses $: C = 12.0 \ u, H = 1.0 \ u, O = 16.0 \ u]$

$A$ spherical balloon of radius $3 \ cm$ containing helium gas has a pressure of $48 \times 10^{-3} \ bar$. At the same temperature,the pressure of a spherical balloon of radius $12 \ cm$ containing the same amount of gas will be........ $\times 10^{-6} \ bar$.

Air entering the lungs ends up in tiny sacs called alveoli. It is from the alveoli that oxygen diffuses into the blood. The average radius of the alveoli is $0.0050 \ cm$ and the air inside contains $14$ per cent oxygen. Assuming that the pressure in the alveoli is $1.0 \ atm$ and the temperature is $37 \ ^oC$,calculate the number of oxygen molecules in one of the alveoli.

What will be the value of the gas constant $R$ when pressure is expressed in $dyne \, m^{-2}$ and volume in $mm^3$?

At temperature $t \, ^oC$,the pressure exerted by $12 \, g$ of an ideal gas in a container of volume $V \, L$ is $1 \, atm$. When the temperature is increased by $10 \, ^oC$ without changing the volume,the pressure increases by $10 \%$. Find the temperature $t$ and volume $V$ in $L$. (Molar mass of the gas = $120 \, g/mol$)

Calculate the volume occupied by $8.8 \,g$ of $CO_{2}$ at $31.1^{\circ} C$ and $1 \,bar$ pressure.
( $R=0.083 \,bar \,L \,K^{-1} \,mol^{-1}$ )