If $28 \ g$ of $N_2$ gas occupies a volume of $10 \ L$ at a pressure of $2.46 \ atm$,the temperature will be ......... $K$.

The compressibility factor of a gas is defined as $Z = PV/RT$. The compressibility factor of an ideal gas is:

If $2 \, \text{moles}$ of an ideal gas occupy a volume of $44.8 \, L$ at a temperature of $546 \, K$,what will be the pressure in $atm$?

At $400 \ K$,an ideal gas is enclosed in a $0.5 \ m^3$ vessel at a pressure of $203 \ kPa$. What is the change in temperature required (in $K$),if it occupies a volume of $0.2 \ m^3$ under a pressure of $304 \ kPa$? (Nearest integer)

Calculate the temperature of $4.0 \, mol$ of a gas occupying $5 \, dm^{3}$ at $3.32 \, bar$.
$(R = 0.083 \, bar \, dm^{3} \, K^{-1} \, mol^{-1})$

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