Equal volumes of two gases which do not react together are enclosed in separate vessels. Their pressures are $100 \ mm$ and $400 \ mm$ respectively. If the two vessels are joined together,then what will be the pressure of the resulting mixture (temperature remaining constant)?

The temperature at which $4 \ mol$ of a gas occupies $5 \ dm^3$ volume at $3.32 \ bar$ pressure is:

Which of the following is equal to $[{\partial P/\partial V}]_T$ for an ideal gas?

At $127 \, ^oC$ temperature,the volume of a gas is $3 \, L$. If the volume of the gas becomes half at constant pressure,calculate the final temperature in Kelvin. (in $, K$)

What is the density of $N_2$ gas at $227\,^\circ C$ and $5.00\ atm$ pressure? (Given: $R = 0.082\ L\ atm\ K^{-1}\ mol^{-1}$)

Consider the figure provided. $1 \ mol$ of an ideal gas is kept in a cylinder,fitted with a piston,at the position $A$,at $18^{\circ} C$. If the piston is moved to position $B$,keeping the temperature unchanged,then '$x$' $L \ atm$ work is done in this reversible process. $x=$ . . . . . . $L \ atm$. (nearest integer) [Given : Absolute temperature $=^{\circ} C + 273.15$,$R=0.08206 \ L \ atm \ mol^{-1} \ K^{-1}$]