$125 \, ml$ of gas $A$ at $0.60 \, atm$ and $150 \, ml$ of gas $B$ at $0.80 \, atm$ pressure at the same temperature are filled in a vessel of $1 \, L$ volume. What will be the total pressure of the mixture at the same temperature in $atm$?

For a diatomic gas,the change in internal energy at constant pressure and the change in internal energy for a unit temperature change are $U_1$ and $U_2$ respectively. Then $U_1 : U_2$ is equal to:

The difference between volume and pressure coefficients of an ideal gas is

According to the kinetic theory of gases,when two molecules of a gas collide with each other,then:

$A$ jar contains a gas and a few drops of water at $T \, K.$ The pressure in the jar is $830 \, mm$ of mercury. The temperature of the jar is reduced by $1\%.$ The saturated vapour pressure of water at the two temperatures are $30 \, mm$ and $25 \, mm$ of mercury. Then the new pressure in the jar will be ..... $mm$ of $Hg$.

$A$ rigid diatomic gas having molar mass $M$ is contained in an insulated container. The container is moving with velocity $V$. If it is stopped suddenly, the change in temperature is ($R$ - gas constant).